Titration Based Problems Random Retrieval

3

Titration Based Problems Random Retrieval

This quiz contains all the questions in the Titration Based Problems section. The website will pick 10 questions at random.

1 / 10

3.94g of potassium hydrogencarbonate was dissolved in deionised water and made up to 100cm3 in a volumetric flask.

10.0cm3 samples were titrated against sulfuric acid solution of concentraion 0.150 mol dm-3.

A mean titre of 11.70cm3 of sulfuric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

2 / 10

2.79g of sodium carbonate was dissolved in deionised water and made up to 250cm3 in a volumetric flask.

20.0cm3 samples were titrated against hydrochloric acid solution of concentraion 0.350 mol dm-3.

A mean titre of 11.80cm3 of hydrochloric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

3 / 10

0.925g of lithium hydroxide was dissolved in deionised water and made up to 250cm3 in a volumetric flask.

25.0cm3 samples were titrated against sulfuric acid solution of concentraion 0.100 mol dm-3.

A mean titre of 13.75cm3 of sulfuric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

4 / 10

1.66g of potassium hydroxide was dissolved in deionised water and made up to 100cm3 in a volumetric flask.

25.0cm3 samples were titrated against nitric acid solution of concentraion 0.300 mol dm-3.

A mean titre of 23.45cm3 of nitric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

5 / 10

2.5g of potassium hydroxide was dissolved in deionised water and made up to 250cm3 in a volumetric flask.

25.0cm3 samples were titrated against nitric acid solution of concentraion 0.150 mol dm-3.

A mean titre of 18.15cm3 of nitric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

6 / 10

Calculate the pH of a solution created by the addition of 30.0cm3 0.100 mol dm-3 lithium hydroxide solution to 35.0 cm3 0.100 mol dm-3 hydrobromic acid solution.

Remember to give your answer to 3 sig.fig.

7 / 10

By titration, it was found that an average titre of 9.90cm3 of 1.00 mol dm-3 solution of potassium carbonate was required to just neutralise a 25.00 cm3 sample of sulfuric acid solution. Calculate the concentraion of the sulfuric acid solution.

The equation for the reaction is

K2CO3(aq)+H2SO4(aq)=>K2SO4(aq)+H2O(aq)+CO2(g)

8 / 10

By titration, it was found that an average titre of 21.25cm3 of 2.450 mol dm-3 solution of sulfuric acid was required to just neutralise a 10.00 cm3 sample of barium hydroxide solution. Calculate the concentraion of the barium hydroxide solution.

The equation for the reaction is

H2SO4(aq)+Ba(OH)2(aq)=>BaSO4(aq)+2H2O(aq)

9 / 10

By titration, it was found that an average titre of 21.30cm3 of 0.100 mol dm-3 solution of sulfuric acid was required to just neutralise a 25.00 cm3 sample of potassium hydroxide solution. Calculate the concentraion of the potassium hydroxide solution.

The equation for the reaction is

2KOH(aq)+H2SO4(aq)=>K2SO4(aq)+H2O(aq)

10 / 10

By titration, it was found that an average titre of 22.85cm3 of 0.300 mol dm-3 solution of nitric acid was required to just neutralise a 25.00 cm3 sample of sodium carbonate solution. Calculate the concentraion of the sodium carbonate solution.

The equation for the reaction is

2HNO3(aq)+Na2CO3(aq)=>2NaNO3(aq)+H2O(aq)+CO2(g)

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Moles & Solutions Random Retrieval

5

Moles & Solutions Random Retrieval

This quiz contains all the questions in the Moles & Solutions section. The website will pick 10 questions at random.

1 / 10

What volume (in cm3) of deionised water would you need to add to 50.0cm3 of ammonia solution to dilute it from a concentration of 10.0 mol dm-3 into a concentration of 1.00 mol dm-3?

2 / 10

What volume (in cm3) of deionised water would you need to add to 100cm3 of hydrochloric acid to dilute it from a concentration of 2.00 mol dm-3 into a concentration of 1.00 mol dm-3?

3 / 10

Calculate the concentration of iodine in a solution of volume 4.80dm3 that contains 250 g of iodine

I=126.9

4 / 10

Calculate the concentration of potassium hydrogencarbonate in a solution of volume 280cm3 that contains 50.0 g of potassium hydrogencarbonate

K=39.1 H=1.0 C=12.0 O=16.0

5 / 10

Calculate the concentration of potassium hydrogencarbonate in a solution of volume 900cm3 that contains 50.0 g of potassium hydrogencarbonate

K=39.1 H=1.0 C=12.0 O=16.0

6 / 10

Calculate the volume of solution in cm3 that would contain 0.200 mol of lithium iodide if the concentration of the solution is 0.800 mol cm-3

7 / 10

Calculate the volume of solution in dm3 that would contain 0.400 mol of copper (II) sulfate if the concentration of the solution is 1.10 mol dm-3

8 / 10

Calculate the volume of solution in dm3 that would contain 0.800 mol of sulfuric acid if the concentration of the solution is 0.200 mol dm-3

9 / 10

Calculate the volume of solution in cm3 that would contain 0.150 mol of chlorate (I) ions if the concentration of the solution is 0.150 mol cm-3

10 / 10

Calculate the number of moles of hydrofluoric acid in a solution of volume 22.45 cm3 and a concentration of 0.250 mol dm-3

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Moles & Gases Random Retrieval

6

Moles & Gases Random Retrieval

This quiz contains all the questions in the Moles & Gases section. The website will pick 10 questions at random.

1 / 10

Calculate the volume of gas (in dm3) of 1.40 mol of sulfur hexafluoride if the gas is at a temperature of 3000K and a pressure of 1000kPa

2 / 10

Calculate the volume of gas (in m3) of 0.500 mol of hydrogen if the gas is at a temperature of 373K and a pressure of 5000Pa

3 / 10

Calculate the volume of gas (in dm3) of 2.00 mol of gaseous ammonia if the gas is at a temperature of 1000K and a pressure of 75000Pa

4 / 10

Calculate the volume of gas (in cm3) of 0.0500 mol of neon if the gas is at a temperature of 273K and a pressure of 505000Pa

5 / 10

Calculate the volume of gas (in dm3) of 0.400 mol of helium if the gas is at a temperature of 273K and a pressure of 50000Pa

6 / 10

Calculate the temperature of a sample of butane (in oC) if 0.110 mol of butane has a volume of 879cm3 and is at a pressure of 700kPa

7 / 10

Calculate the temperature of a sample of nitrogen (in oC) if 0.160 mol of nitrogen has a volume of 1850cm3 and is at a pressure of 120000Pa

8 / 10

Calculate the temperature of a sample of fluorine (in oC) if 0.890 mol of fluorine has a volume of 125dm3 and is at a pressure of 95000Pa

9 / 10

Calculate the temperature of a sample of neon (in K) if 2.00 mol of neon has a volume of 24.00dm3 and is at a pressure of 50000Pa

10 / 10

Calculate the number of moles of gas present at r.t.p in 6000 cm3 of methane.

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Moles & Masses Random Retrieval

10

Moles & Masses Random Retrieval

This quiz contains all the questions in the Moles & Masses section. The website will pick 10 questions at random.

1 / 10

Calculate the number of moles of magnesium hydroxide if you have 62.0 g of magnesium hydroxide

H=1.0 C=12.0 O=16.0

2 / 10

Calculate the number of moles of fluorine if you have 76.0 g of fluorine

F=19.0

3 / 10

Calculate the number of moles of glucose if you have 36.0 g of glucose

H=1.00 C=12.0 O=16.0

4 / 10

Calculate the number of moles of FeSO4 . 7H2O if you have 45.6 g of FeSO4 . 7H2O

S=32.1 Fe=55.8 O=16.0 H=1.0

5 / 10

Calculate the number of moles of N2 if you have 28.0 g of N2

N=14.0

6 / 10

Calculate the number of moles of Al2(SO4)3 if you have 17.1 g of Al2(SO4)3

 

S=32.1 Al=27.0 O=16.0

7 / 10

Calculate the number of moles of H2SO4 if you have 27.0 g of H2SO4

S=32.1 H=1.0 O=16.0

8 / 10

Calculate the mass of iodine that you would have if you had 0.0500 mol of iodine

I=126.9

9 / 10

Calculate the mass of fluorine that you would have if you had 1.75 mol of fluorine

F=19.0

10 / 10

Calculate the mass of P2O5 that you would have if you had 0.100 mol of P2O5

P=31.0 O=16.0

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Moles Sets Random Retrieval

5

Moles Sets Random Retrieval

This quiz contains all the questions in the Moles Sets section. The website will pick 10 questions at random.

1 / 10

Barium hydroxide solution will neutralise hydrochloric acid according to the equation

Ba(OH)2+2HCl =>BaCl2+2H2O

What volume of 0.1mol dm-3 HCl will neutralise 250 cm3 of 0.2mol dm-3 Ba(OH)2?

2 / 10

Which solution of NaCl is the most concentrated?

3 / 10

How many moles of molecules are present in 48.0 dm3 of butane? (all volumes measured at r.t.p.)

4 / 10

KClO3 => KClO4 + KCl

5 / 10

The empirical formula of a compound:

6 / 10

Work out the names of each of the following compounds from their formula. Use the data sheet Names & Formulae of Some Common Ions

Formulae are Case Sensitive.

Remember to use regular numbers in formulae e.g. H2O not H2O

HBr

7 / 10

silicon (IV) fluoride

8 / 10

sulfur (VI) fluoride

9 / 10

iron (III) sulfate

10 / 10

Calculate the relative molecular mass (formula mass) of zinc hydroxide, Zn(OH)2

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Chemistry Random Retrieval Y13

34

Chemistry Year 13 Random Retrieval

This quiz contains all the questions in the year 13 chemistry section. The website will pick 10 questions at random.

1 / 10

What is the organic product when benzene reacts with ethanoyl chloride in the presence of aluminium chloride?

2 / 10

Which types of change are involved in this sequence of reactions, though not necessarily in the order listed?

CH3CO-C6H5 -> CH3CO-C6H4-NO2 -> CH3CHOH-C6H4-NO2 -> CH3CH(OCOCH3)-C6H4-NO2

(i) esterification

(ii) reduction

(iii) nitration

(iv) hydrolysis

3 / 10

In a peptide made up of a sequence of four amino acids the number of peptide bonds is:

4 / 10

When 0.08 g magnesium ribbon reacts with 50 cm3 of 2.00 mol dm-3 hydrochloric acid the reaction produces 80 cm3 gas in 400 seconds at room temperature and pressure but then stops. On repeating the reaction under the same conditions with 0.08 g magnesium ribbon and 100 cm3 of 1.00 mol dm-3 hydrochloric acid the outcome is that the reaction:

5 / 10

What are the units of k for this reaction?

[1] s-1

[2] mol-1 dm3 s-1

[3] mol-2 dm6 s-1

[4] mol-3 dm9 s-1

6 / 10

Which graph represents the disappearance of a reactant that displays first order kinetics?

7 / 10

Kp = 4 atm for the dissociation of N2O4 at 350 K when the equilibrium is described by this equation.

N2O4(g) <=> 2NO2(g)

What is the value of Kp for this equilibrium:

2NO2(g) <=> N2O4(g)?

8 / 10

Consider the following equilibrium for the reaction that generates hydrogen for use in the Haber-Bosch Process:

CH4(g) + H2O(g) <=>CO(g) + 3H2(g)

100 mol of CH4 was mixed with 100 mol of H2O and 200 mol of H2.The mixture was given time to reach equilibrium. At this point, 350 mol of H2 was present in the mixture. The pressure inside the 1.20 m3 vessel was measured as 400 kPa

Calculate the value of Kp (in units: kPa2) under these conditions.

9 / 10

For this question, look at the resource, ‘A Selection of Standard Electrode Potentials’ (‘A Selection of Standard Electrode Potentials’can be found in TOOLS>Data Sheets)

Is Cu2+(aq) capable of oxidising Ag(s)?

10 / 10

Consider a cell constructed from the following half-cells:

Zn2+(aq) + 2e- <=> Zn(s) Eϴ/V = -0.76

Cu2+(aq) + 2e- <=>Cu(s) Eϴ/V = +0.34

Which half-cell will form the cathode in this cell? Think very carefully about the definition of a cathode!

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7

Physical Chemistry & Transition Elements Random Retrieval

This quiz contains all the questions in the Physical Chemistry & Transition Elements section. The website will pick 10 questions at random.

1 / 10

For this question, look at the resource, ‘A Selection of Standard Electrode Potentials’ (‘A Selection of Standard Electrode Potentials’can be found in TOOLS>Data Sheets)

Which chemical species is most resistant to oxidation?

2 / 10

Consider a cell constructed from the following half-cells:

Mg2+(aq) + 2e- <=> Mg(s) Eϴcell/V = -2.37

Ag+(aq) + e- <=> Ag(s) Eϴcell/V = +0.80

If the solution of Mg2+(aq) was 2.00 mol dm-3, would you expect to see a greater or smaller value of Eϴcell/V than you would if the cell was set-up under standard conditions?

3 / 10

Work out the ratio of the species in the following half-equation.

Cu => Cu2+ + e-

4 / 10

Using oxidation numbers (states) work out the ratio of the species in the following half-equation.

S2O32- + H2O => SO42- + H+ + e-

5 / 10

Using oxidation numbers (states) work out the ratio of the species in the following half-equation.

I2 + e- => I-

6 / 10

Which of these complex ions acts as an acid in aqueous solution?

(i) [Ni(NH3)6]2+

(ii) [Al(H2O)2(OH)4]-

(iii) [Ag(NH3)2]+

(iv) [Cr(H2O)6]3+

7 / 10

Which types of chemical bonding feature in crystals of the compound K2[Ni(CN)4]?

(i) ionic bonding

(ii) covalent bonding

(iii) dative covalent bonding

(iv) metallic bonding

8 / 10

For the following equilibrium Kc = 25.0 mol-2 dm6 at a particular temperature.

CO(g) + 2H2(g) <=> CH3OH(g)

Which of these changes of conditions alter the value of Kc?

(i)Raising the concentration of hydrogen

(ii)Adding a catalyst

(iii)Raising the pressure

(iv)Lowering the temperature

9 / 10

Consider the following reaction:

2NO2(g) + F2(g) => 2NO2F(g)

The rate equation was found, by experiment:

rate = k [NO2] [F2]

Which of the following statements is/are true?

(i) The mechanism has more than one step

(ii) Doubling [NO2] doubles the rate of the reaction

(iii) NO2 is produced in one of the steps

(iv) The mechanism has only one step

10 / 10

The activation energy for the reaction of cobalt metal with aqueous S2O82- ions is close to 50 kJ mol-1. The rate of reaction for the metal when a cylinder of cobalt metal rotates rapidly in a solution of aqueous S2O82- ions at 15oC is 1.80 mg min-1. This suggests that at 25oC the rate of reaction would be about:

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10

Organic Chemistry & Analysis Random Retrieval

This quiz contains all the questions in the Organic Chemistry & Analysis section. The website will pick 10 questions at random.

1 / 10

Which of these compounds are chiral?

(i) propan-1-ol,

(ii) propan-2-ol,

(iii) butan-1-ol,

(iv) butan-2-ol

2 / 10

Which of these compounds are chiral?

(i) CH2Cl2

(ii) CH2ClBr

(iii)CHCl2F

(iv) CH3CHClBr

3 / 10

Which of these compounds are functional group isomers of

HCO2CH2CH2CH3?

(i) ethyl ethanoate,

(ii) 2-methylpropanoic acid,

(iii) methyl propanoate,

(iv) butanoic acid

4 / 10

The rate equation for the reaction of hydroxide ions with 2-bromo-2-methylpropane takes the form:

rate = k[C4H9Br].

This indicates that:

(i) the rate determining step involves hydroxide ions

(ii) doubling the concentration of the halogenoalkane doubles the rate of reaction

(iii) the reaction takes place in one step

(iv) the reaction takes place by the SN1 mechanism (a 2 step mechanism)

5 / 10

The reaction of benzene with ethanoyl chloride in the presence of aluminium chloride

(i) involves CH3-CO+ as an intermediate

(ii) forms C6H5-CO-CH3

(iii) is a substitution reaction

(iv) involves nucleophilic attack on benzene

6 / 10

Which statement helps to explain why propene react with hydrogen bromide to form mainly 2-bromopropane and much less 1-bromopropane?

7 / 10

Which of these chemical species are nucleophiles with react with halogenoalkanes?

(i) cyanide ions

(ii) hydroxide ions

(iii) ammonia molecules

(iv) ammonium ions

8 / 10

In which of these reactions between pairs of reagents is the bond breaking homolytic?

(i) butan-1-ol with sodium bromide and concentrated sulfuric acid

(ii) catalytic cracking of hydrocarbons

(iii) bromine with ethene

(iv) bromine with hexane

9 / 10

If the paracetamol molecule shown below is hydrolysed in hot dilute hydrochloric acid, what are the main organic products?

10 / 10

Which types of change are involved in this sequence of reactions, though not necessarily in the order listed?

CH3CO-C6H5 -> CH3CO-C6H4-NO2 -> CH3CHOH-C6H4-NO2 -> CH3CH(OCOCH3)-C6H4-NO2

(i) esterification

(ii) reduction

(iii) nitration

(iv) hydrolysis

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Chemistry Random Retrieval Y12

59

Chemistry Year 12 Random Retrieval

This quiz contains all the questions in the year 12 chemistry section. The website will pick 10 questions at random.

1 / 10

The peak with the largest mass to charge ratio in the mass spectrum of an alkane is detected at mass-to-charge ratio = 58.

This shows that the hydrocarbon:

2 / 10


Choose one of the following options:

3 / 10

The reaction of calcium with water produces:

4 / 10

Using enthalpies of formation ΔfH, calculate the enthalpy change for the following hydration process.

Na2S2O3(s) + 5H2O(l) => Na2S2O3•5H2O(s)

Select the data from the 'Selection of Enthalpies of Formation and Combustion' shown above.

If this question was generated from Random Retrieval, this data can also be found in TOOLS>Data Sheets.

5 / 10

Each of these statements is true. From which statement is it possible to predict, by application of Le Chatelier's principle that the solubility of sodium hydroxide increases with temperature?

6 / 10

A small crystal of iodine is dissolved in hexane to give a violet coloured solution. After adding an equal volume of colourless, aqueous potassium iodide and shaking, the system reaches equilibrium with the hexane layer floating on top of the aqueous layer. At equilibrium:

(i) the concentrations of iodine in the two layers are the same

(ii) the iodine in the hexane turns brown

(iii) the iodine molecules stop moving between the two layers

(iv) the concentrations in each layer stop changing

7 / 10

What is the electronic configuration of scandium? Enter your answer in the following format 1s2 2s2 etc. (note the space between each sub-shell!) Follow the aufbau order of sub-shell filling.

8 / 10

Calculate the volume of oxygen gas formed on strongly heating 3.40 g sodium nitrate which decomposes according to this equation:

2NaNO3(s) -> 2NaNO2(s) + O2(g)

Assume that the volume of 1 mol of any gas is 24 000 cm3 under the conditions of the experiment.

9 / 10

In which of these molecules do the intermolecular forces arise largely from attractions between permanent dipoles?

10 / 10

Hydrogen is oxidised when it reacts with:

(i) oxygen to form water

(ii) nitrogen to form ammonia

(iii) chlorine to form hydrogen chloride

(iv) sodium to form sodium hydride

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19

Foundations in Chemistry Random Retrieval

This quiz contains all the questions in the Foundations in Chemistry section. The website will pick 10 questions at random.

1 / 10

Hydrogen is oxidised when it reacts with:

(i) oxygen to form water

(ii) nitrogen to form ammonia

(iii) chlorine to form hydrogen chloride

(iv) sodium to form sodium hydride

2 / 10

The oxidation number of sulfur in sulfuric acid, H2SO4, is:

3 / 10

In a titration, 25 cm3 of 0.100 mol dm-3 potassium hydroxide was neutralised by 12.5 cm3 dilute nitric acid. What was the concentration of the nitric acid?

4 / 10

Which of these elements has a relatively low boiling point (below 500 oC)?

5 / 10

In a close-packed metal structure:

(i) there are no spaces between the atoms

(ii) the atoms are arranged in layers

(iii) the crystal breaks if the layers slide past each other

(iv) each atom touches 12 nearest neighbours.

6 / 10

Which of these statements are true for the hydrides of group 5: NH3, PH3, AsH3 and SbH3:

(i) the molecules decrease in size down the group

(ii) the boiling point of ammonia is higher than expected from the general trend in values down the group

(iii) none of the molecules is polar

(iv) only ammonia is affected by hydrogen bonding

7 / 10

Using the basic rules of VSEPR, what would you expect the bond angle to be in H2S?

8 / 10

Which of these molecules are overall polar?

(i) CH3Cl

(ii) CH2Cl2

(iii) CHCl3

(iv) CCl4

9 / 10

In the formula of water, H-O-H, the lines represent:

(i) shared pairs of electrons

(ii) dative bonds

(iii) covalent bonds

(iv) hydrogen bonds

10 / 10

How many chloride ions touch each sodium ion in the crystal structure of sodium chloride?

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8

Period Table & Energy Random Retrieval

This quiz contains all the questions in the Period Table & Energy section. The website will pick 10 questions at random.

1 / 10

This is the equilibrium in a solution of bromine in water:

Br2(aq) + H2O(l) <=> HOBr(aq) + H+(aq) + Br-(aq)

The orange colour of bromine disappears on adding

(i) sodium bromide

(ii) water

(iii) dilute hydrochloric acid

(iv) sodium hydroxide solution

2 / 10

The total O.N. of all the halogen atoms in these compounds ClO-, BrO-, ICl, XeF4 is:

3 / 10

Chlorine disproportionates when it reacts with:

4 / 10

The carbonates of group 2 metals (M):

(i) have the formula of the form MCO3

(ii) are insoluble in water

(iii) become more difficult to decompose on heating down the group

(iv) decompose on heating to the metal and carbon dioxide

5 / 10

What is the oxidation number of CARBON in

CCl4

6 / 10

What is the oxidation number of MANGANESE in

MnO4-

7 / 10

What is the oxidation number of OSMIUM in

OsO4

8 / 10

What is the oxidation number of CARBON in

CH4

9 / 10

Which of these statements about atomic and ionic radii are true?

(i) Atomic radii increase down group 2

(ii) Ionic radii increase down group 7

(iii) Atomic radii decrease across period 3

(iv) In period 3 the ionic radii are smaller than the atomic radii

10 / 10

An element which is a solid at room temperature consisting of molecules is:

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20

Core Organic Chemistry Random Retrieval

This quiz contains all the questions in the Core Organic Chemistry section. The website will pick 10 questions at random.

1 / 10

2 / 10

3 / 10

How many functional group isomers of C3H6O2 are there?

It's really difficult to get all of these structures, so don't panic if you miss some. Just spend some time sketching out all the possibilities and remembering some simple rules, e.g carbon forms 4 bonds, oxygen forms 2 etc. Be creative!

4 / 10

A compound X with the molecular formula C4H10O has a broad peak in its IR spectrum at 3500cm-1.

Oxidation of X with excess potassium dichromate(VI) gives a product Y which is not an acid and does not reduce Fehling's solution.

Y has a strong peak in its IR spectrum at 1700cm-1.

Identify X and Y. (See also the data in question 9.)

5 / 10

This procedure produces a white precipitate which dissolves easily in dilute ammonia solution: heating C4H9X for a few minutes with aqueous alkali, then acidifying the mixture with dilute nitric acid and adding silver nitrate. This shows that X is:

6 / 10

What are the conditions for converting 1,2-dichlorethane into ethane-1,2-diol?

7 / 10

Which reagent can be used to convert butan-1-ol to but-1-ene?

8 / 10

What is the H-C-H bond angle in ethene?

9 / 10

What is the name for this structure:

CH3CH(CH3)CH(CH3)CH2CH3?

10 / 10

Which of these hydrocarbons is an alkane?

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Chemistry Year 12 Random Retrieval

59

Chemistry Year 12 Random Retrieval

This quiz contains all the questions in the year 12 chemistry section. The website will pick 10 questions at random.

1 / 10

Which of these alkenes will produce the largest %yield of 2-bromopentane when it is reacted with hydrogen bromide?

2 / 10

Which of these alcohols is a tertiary alcohol?

(i) CH3CH2CHOHCH3

(ii) CH3CH(CH3)CHOHCH3

(iii) CH3C(CH3)2CH2CHOHCH3

(iv) (CH3)3COH

3 / 10


Choose one of the following options:

4 / 10

A white crystalline solid gives a pale green colour in a flame. Adding silver nitrate to an acidified solution of the solid produces a white precipitate. The solid is:

5 / 10

Chlorine disproportionates when it reacts with:

6 / 10

How many electrons are there in an oxide ion?

7 / 10

How many sulfate ions are there in 0.01 mol aluminium sulfate?

(The Avogadro constant = 6.02 x 1023 mol-1)

8 / 10

How many shared pairs of electrons are there in an ethene molecule, C2H4?

9 / 10

What is the bond angle found in water?

10 / 10

In the family of hydrocarbons called alkanes:

(i) the boiling points of the straight chain compounds rise as the number of carbon atoms increases

(ii) the intermolecular forces arise from attractions between temporary dipoles

(iii) in any pair of isomers the compound with the more highly branched molecules has the lower boiling point

(iv) the unbranched compounds are all liquids at room temperature.

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Chemistry Year 13 Random Retrieval

34

Chemistry Year 13 Random Retrieval

This quiz contains all the questions in the year 13 chemistry section. The website will pick 10 questions at random.

1 / 10

The main forces which hold a coiled protein chain into an alpha-helix are:

2 / 10

Which of these phrases describes the tertiary structure of a protein?

3 / 10

Which of these characteristics of polymers accounts for the difference between low density and high density poly(ethene)?

[1] the average length of the polymer chains

[2] the type of intermolecular (interchain) forces

[3] the number and size of bulky side groups

[4] the extent of chain branching

4 / 10

Step 5:

5 / 10

How many peaks would you expect to see in the 13C spectrym of 3-propyl aminobenzene?

 

6 / 10

What enthalpy change is represented by the following equation?

2Na(s) + ½ O2(g)=> Na2O(s)

7 / 10

From your calculation of ΔG in question 8, decide whether the reaction between high pressure steam and methane will be feasible at 1500oC.

If this question is from a Random Retrieval, you can also carry out this calculation of Gibbs Energy change, ΔG by first working out values for ΔSƟ and ΔHƟ by selecting the appropriate data from the ‘Selection of Thermodynamic Data’ in TOOLS.

8 / 10

Which first-row d-block element forms an oxide used as the catalyst in the synthesis of sulfur trioxide from sulfur dioxide and oxygen?

9 / 10

For this question, look at the resource, ‘A Selection of Standard Electrode Potentials’ (‘A Selection of Standard Electrode Potentials’can be found in TOOLS>Data Sheets)

Which chemical species is most resistant to reduction?

10 / 10

For this question, look at the resource, ‘A Selection of Standard Electrode Potentials’ (‘A Selection of Standard Electrode Potentials’can be found in TOOLS>Data Sheets)?

Can MnO4-(aq) oxidise water into H2O2(aq) in acidic condition?

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Foundations in Chemistry Random Retrieval

19

Foundations in Chemistry Random Retrieval

This quiz contains all the questions in the Foundations in Chemistry section. The website will pick 10 questions at random.

1 / 10

What volume of 0.10 mol dm-3 hydrochloric acid is needed to neutralise 20.0 cm3 of 0.05 mol dm-3 barium hydroxide?

2 / 10

Which of these compounds consists of a giant structure of ions?

3 / 10

Which of the following is not a typical property of most metals:

4 / 10

Which of these true statements can help to explain why magnesium has a higher melting point than sodium:

(i) magnesium atoms/ions are smaller than sodium atoms/ions

(ii) the metallic bonds are stronger in magnesium than in sodium

(iii) a magnesium atoms contributes two bonding electrons not one

(iv) the first ionisation energy is higher for magnesium than for sodium.

5 / 10

In which of these solids are there two types of bonding: one strong and one weak?

(i) diamond

(ii) ice

(iii) sodium chloride

(iv) graphite

6 / 10

Which of these elements consist of a giant structure of atoms joined by covalent bonding?

(i) graphite

(ii) sulfur

(iii) diamond

(iv) iodine

7 / 10

8 / 10

Calculate the volume of oxygen gas formed on strongly heating 3.40 g sodium nitrate which decomposes according to this equation:

2NaNO3(s) -> 2NaNO2(s) + O2(g)

Assume that the volume of 1 mol of any gas is 24 000 cm3 under the conditions of the experiment.

9 / 10

What is the electronic configuration of sulfide? Enter your answer in the following format 1s2 2s2 etc. (note the space between each sub-shell!) Follow the aufbau order of sub-shell filling.

10 / 10

E represents an atom of an element in the equation: E(g) -> E+(g) + e Which of these statements is/are true:

(i) the element must be a metal

(ii) the enthalpy change for this process is the first ionisation energy of the element

(iii) the element must be a gas at room temperature.

(iv) this process occurs in a mass spectrometer used to analyse the element

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