Titration Based Problems Random Retrieval

2

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

2.82g of lithium carbonate was dissolved in deionised water and made up to 250cm3 in a volumetric flask.

10.0cm3 samples were titrated against hydrochloric acid solution of concentraion 0.100 mol dm-3.

A mean titre of 28.70cm3 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!)

2 / 10

Calculate the pH of a solution created by the addition of 49.0cm3 0.250 mol dm-3 barium hydroxide (Ba(OH)2) solution to 100 cm3 0.250 mol dm-3 chloric (VII) acid solution.

Remember to give your answer to 3 sig.fig.

3 / 10

Calculate the pH of a solution created by the addition of 20.0cm3 0.200 mol dm-3 potassium hydroxide solution to 50.0 cm3 0.100 mol dm-3 nitric acid solution.

Remember to give your answer to 3 sig.fig.

4 / 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)

5 / 10

By titration, it was found that an average titre of 28.05cm3 of 0.100 mol dm-3 solution of potassium hydroxide was required to just neutralise a 25.00 cm3 sample of phosphoric acid solution. Calculate the concentraion of the phosphoric acid solution.

The equation for the reaction is

3KOH(aq)+H3PO4(aq)=>K3PO4(aq)+3H2O(aq)

6 / 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)

7 / 10

By titration, it was found that an average titre of 28.80cm3 of 2.00 mol dm-3 solution of potassium carbonate was required to just neutralise a 50.00 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 21.85cm3 of 0.200 mol dm-3 solution of potassium hydroxide was required to just neutralise a 10.00 cm3 sample of phosphoric acid solution. Calculate the concentraion of the phosphoric acid solution.

The equation for the reaction is

3KOH(aq)+H3PO4(aq)=>K3PO4(aq)+3H2O(aq)

9 / 10

By titration, it was found that an average titre of 19.10cm3 of 0.250 mol dm-3 solution of sulfuric acid was required to just neutralise a 10.00 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 22.25cm3 of 0.100 mol dm-3 solution of hydrochloric acid was required to just neutralise a 20.00 cm3 sample of lithium hydroxide solution. Calculate the concentraion of the lithium hydroxide solution.

The equation for the reaction is

LiOH(aq)+HCl(aq)=>LiCl(aq)+H2O(aq)

 

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Moles & Solutions Random Retrieval

3

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

Calculate the concentration of HCl in a solution of volume 1.25dm3 that contains 460 g of HCl

H=1 Cl=35.5

2 / 10

Calculate the concentration of Al2(SO4)3 in a solution of volume 2.26dm3 that contains 500 g of Al2(SO4)3

S=32.1 Al=27.0 O=16.0

3 / 10

Calculate the concentration of barium nitrate in a solution of volume 19.85cm3 that contains 4.82 g of barium nitrate

Ba=137.3 N=14.0 O=16.0

4 / 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

5 / 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

6 / 10

Calculate the volume of solution in cm3 that would contain 0.450 mol of Ag+ ions if the concentration of the solution is 0.400 mol cm-3

7 / 10

Calculate the volume of solution in cm3 that would contain 1.12 mol of ammonia if the concentration of the solution is 6.50 mol cm-3

8 / 10

Calculate the volume of solution in dm3 that would contain 0.200 mol of NO3- ions if the concentration of the solution is 1.85 mol dm-3

9 / 10

Calculate the number of moles of silver nitrate in a solution of volume 1.10 dm3 and a concentration of 1.30 mol dm-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

4

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 1.20 mol of sulfur hexafluoride if the gas is at a temperature of 750K and a pressure of 150kPa

2 / 10

Calculate the volume of gas (in cm3) of 0.175 mol of nitrogen if the gas is at a temperature of 800K and a pressure of 1000kPa

3 / 10

Calculate the volume of gas (in m3) of 7.00 mol of hydrogen chloride if the gas is at a temperature of 3000K and a pressure of 1000kPa

4 / 10

Calculate the number of moles of gas present at r.t.p in 700 cm3 of butane.

5 / 10

Calculate the number of moles of gas present at r.t.p in 6.6 m3 of helium.

6 / 10

Calculate the number of moles of gas present at r.t.p in 18.0 dm3 of propane.

7 / 10

Calculate the number of moles of gas present at r.t.p in 3000 cm3 of oxygen.

8 / 10

Calculate the number of moles of gas present at r.t.p in 0.600 dm3 of fluorine.

9 / 10

Calculate the number of moles of gas present at r.t.p in 0.200 m3 of methane.

10 / 10

Calculate the number of moles of gas present at r.t.p in 40.0 dm3 of hydrogen chloride.

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Moles & Masses Random Retrieval

8

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 hydrogen if you have 6.00 g of hydrogen

H=1.0

2 / 10

Calculate the number of moles of phosphorus (V) oxide (P4O10) if you have 80.0 g of phosphorus (V) oxide (P4O10)

P=31.0 O=16.0

3 / 10

Calculate the number of moles of F2 if you have 9.50 g of F2

F=19.0

4 / 10

Calculate the number of moles of Mg(OH)2 if you have 87.5 g of Mg(OH)2

Mg=24.3 H=1.00 O=16.0

5 / 10

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

C=12.0 H=1.0

6 / 10

Calculate the mass of phosphorus (V) oxide (P4O10) that you would have if you had 1.25 mol of phosphorus (V) oxide (P4O10)

P=31.0 O=16.0

7 / 10

Calculate the mass of aluminium sulfate that you would have if you had 0.860 mol of aluminium sulfate

S=32.1 Al=27.0 O=16.0

8 / 10

Calculate the mass of sodium that you would have if you had 3.00 mol of sodium

Na=23.0

9 / 10

Calculate the mass of Ba(NO3)2 that you would have if you had 0.900 mol of Ba(NO3)2

Ba=137.3 N=14.0 O=16.0

10 / 10

Calculate the mass of FeSO4 . 7H2O that you would have if you had 3.00 mol of FeSO4 . 7H2O

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

 

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Moles Sets Random Retrieval

3

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

If 1 dm3 of 0.1 mol dm-3 Ba(OH)2 neutralises 0.5 dm3 of dilute hydrochloric acid, what is the concentration of the acid?

2 / 10

What volume (measured under r.t.p. of oxygen will be produced by complete thermal decomposition of 4.25g of sodium nitrate?

2NaNO3 => 2NaNO2 + O2

3 / 10

How many moles of molecules are present in 2.40 dm3 of argon? (all volumes measured at r.t.p.)

4 / 10

The mass of 0.250 moles of LiOH is:

5 / 10

Ca3N2

6 / 10

silver nitrate

7 / 10

zinc oxide

8 / 10

How many carbon-12 atoms would have the same mass as 1 Ag atom? Enter a whole number.

9 / 10

Neon (accurate relative atomic mass = 20.18) is made up of three isotopes: Ne-20, Ne-21 and Ne-22.

One of these makes up 90.92% of the element. Which one?

10 / 10

Identify the element (write the symbol) if an atom of Z is one-third of the mass of a 12C atom.

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Chemistry Random Retrieval Y13

26

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 systematic name of the following molecule?

CH3CH2CH2C(NH2)CHCH3

2 / 10

Which of these molecules does NOT consist of one or more chains of amino acids?

(i) The hormone insulin

(ii) The filaments in muscle fibres

(iii) The enzyme in saliva, amylase

(iv) The genetic material, DNA

3 / 10

Which of these compounds are chiral?

(i) propan-1-ol,

(ii) propan-2-ol,

(iii) butan-1-ol,

(iv) butan-2-ol

4 / 10

Consider the values of the equilibrium constant for this reversible reaction:

H2(g) +I2(g) <=> 2HI(g)

Temperature: 500K, value of Kc = 160

Temperature: 1000K, value of Kc = 54.

This information shows that:

(i) HI decomposes rapidly at 500 K

(ii) Raising the temperature causes the equilibrium to shift to the left

(iii) Raising the pressure causes the equilibrium to shift to the right

(iv) The reaction is exothermic

5 / 10

Consider the following equilibrium:

2SO2(g) + O2(g) <=>2SO3(g)

8.00 mol of SO2 was mixed with 5.00 mol of O2 and the mixture sealed in a heated vessel of volume of 1.00 dm3. The mixture was left until no further observable change in composition took place. At this point, 2.00 mol of O2 was present in the mixture and the pressure was recorded as 200 kPa.

Calculate the value Kc (in units: mol-1 dm3) under these conditions.

6 / 10

Look at the chemical equation below.

CH4(g) + H2O(g)=> CO(g)+ 3H2(g)

By selecting the appropriate data from the ‘Selection of Thermodynamic Data’ in TOOLS, calculate the enthalpy change ΔHƟ for the process. Take care with states!

7 / 10

Which of the first-row d-block metals forms aqueous ions which are mauve in the +2 state, green in the +3 state, blue in the +4 state and yellow in the +5 state?

8 / 10

Which first-row d-block metal has the main oxidation state +2 and forms colourless compounds?

9 / 10

Which first-row d-block metal forms hydrated ions in the +3 state which undergo a ligand exchange reaction to form a deep red complex ion with thiocyanate ions, SCN-.

10 / 10

Thinking carefully about the definitions of anode and cathode in electrochemical cells, an anode is defined as (CARE!):

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2

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

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)

Under standard conditions, can Mg2+(aq) be reduced to Mg(s) by Ca(s)?

3 / 10

What is the value of Eϴcell/V observed for a cell constructed from the following half-cells. (These are the half-cells that are put together in a car battery (6 cells in series)?

PbSO4(s) + 2e- <=> Pb(s) + SO42-(aq) Eϴ/V = -0.36

PbO2(s) + SO42-(aq)+4H(aq) + 2e- <=> PbSO4(s) + 2H2O(l) Eϴ/V = +1.69

4 / 10

What is the value of Eϴcell/V observed for a cell constructed from the following half-cells? These half-cells are those involved in Hydrogen Fuel Cells when operated in acidic conditions?

H+(aq) + e-<=> ½H2(g) (acidic conditions) Eϴ/V = 0.00

O2(g)+ 4H+(aq) + 4e-<=>2H2O(g) (acidic conditions) Eϴ/V = +1.23

5 / 10

What is the value of Eϴcell/V observed for a cell constructed from the following half-cells?

Fe3+(aq) + e- <=> Fe2+(aq) Eϴ/V = +0.77

MnO4-(aq) + 8H+(aq) + 5e- <=> Mn2+(aq) + 4H2O(aq) Eϴ/V = +1.51

6 / 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

7 / 10

If pressures are measured in pascals (Pa) what are the units of Kp for this equilibrium:

2H2(g) + O2(g) <=> 2H2O(g)

8 / 10

By inspection of this experimental data, what is the rate equation for this reaction?

9 / 10

Which of these are examples of kinetic stability?

(i) A solution of hydrogen peroxide can be stored at room temperature

(ii) Hydrogen does not ignite in air at room temperature

(iii) Aluminium does not corrode in moist air

(iv) Magnesium oxide does not decompose on heating

10 / 10

The activation energy for the reaction of sodium thiosulfate with acid is close to 50 kJ mol-1. Mixing a measured volumes of sodium thiosulfate solution and hydrochloric acid at 30oC produces a certain amount of sulfur in 120 seconds.

Repeating the experiment with all the conditions the same except the temperature is 40 oC produces the same amount of sulfur in:

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6

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

This is the 1H NMR spectrum of:

2 / 10

Which of these compounds are chiral?

(i) CH2Cl2

(ii) CH2ClBr

(iii)CHCl2F

(iv) CH3CHClBr

3 / 10

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

(i) cyanide ions

(ii) hydroxide ions

(iii) ammonia molecules

(iv) ammonium ions

4 / 10

In which of these organic compounds are all the bonds non-polar?

(i) 1-bromobutane

(ii) butene

(iii) butan-2-ol

(iv) butane

5 / 10

Step 1:

6 / 10

Which of these compounds are solids at room temperature?

(i) propane

(ii) propanoic acid

(iii) propylamine

(iv) 2-aminopropanoic acid

7 / 10

Which of the following molecules would you predict to be the most soluble in water?

8 / 10

Which types of change are involved in this sequence of changes (but not necessarily in the order listed)?

CH3CH2CH2OH -> CH3CH2CHO -> CH3CH2CO2H -> CH3CH2CO2CH2CH3

(i) hydrolysis

(ii) esterification

(iii) acid-base

(iv) oxidation

9 / 10

The reaction of propanone with HCN in the presence of some KCN is an example of:

10 / 10

Which types of alcohol, when heated under reflux with acidified potassium dichromate(VI), turn the colour of the solution from orange to green?

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Chemistry Random Retrieval Y12

51

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 formulae represents 2,2-dimethylpentane?

(i) CH3C(CH3)2CH2CH2CH3

(ii) CH3CH2C(CH3)2CH2CH3

(iii) CH3CH2CH2C(CH3)2CH3

(iv) CH3CH2CH2CH2CH(CH3)2

2 / 10

What type of reaction takes place on passing the vapour of ethanol over hot aluminium oxide? (Water and an alkene are produced)

3 / 10

What is the oxidation number of NITROGEN in

NH3

4 / 10

What is the electronic configuration of carbon?

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.

5 / 10

A chloride ion and an argon atom have the same:

(i) number of protons

(ii) number of electrons

(iii) atomic number

(iv) electron configuration

6 / 10

Which of these sets of properties is that of a substance which is molecular?

7 / 10

What is the bond angle found in water?

8 / 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.

9 / 10

In which of these elements are the atoms or molecules closely packed but free to move around sliding past each other at room temperature?

(i) mercury

(ii) argon

(iii) bromine

(iv) iodine

10 / 10

Which of these acids is only slightly ionised in aqueous solution?

(i) hydrochloric acid

(ii) nitric acid

(iii) sulfuric acid

(iv) ethanoic acid

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17

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

In which of the following industrial conversions is a chemical species (atoms, molecule or ion) oxidised to give the element:

(i) iron ore oxide to iron

(ii) potassium iodate(V) to iodine

(iii) copper(II) sulfate to copper

(iv) sodium chloride to chlorine

2 / 10

What is the concentration of a solution of sodium hydroxide that is made by dissolving 20.0g of the solid in water and making the solution up to 250 cm3? (Relative atomic masses: Na = 23, O = 16, H = 1)

3 / 10

The ionic equation for a neutralisation reaction is:

4 / 10

Which of these gases behaves very much like an ideal gas at room temperature and pressure?

(i) helium

(ii) oxygen

(iii) hydrogen

(iv) butane

5 / 10

What is the bond angle found in BeCl2?

6 / 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

7 / 10

An element M has two electrons in its outer shell. An element X has seven electrons in its outer shell. What is the likely formula of the compound of X and Y?

8 / 10

How many partially filled orbitals are there in the nitrogen atom?

9 / 10

How many filled orbitals are there in the neon atom?

10 / 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.

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4

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

The synthesis of sulfur trioxide takes place at 380 oC in the presence of a catalyst made from vanadium(V) oxide.

2SO2(g) + O2(g) <=> 2SO3(g) Standard enthalpy change = -297 kJ mol-1

Reasons for not choosing a lower temperature are that:

(i) the product condenses to a solid at a lower temperature

(ii) the proportion of SO3(g) at equilibrium falls if the temperature falls

(iii) the reaction is exothermic

(iv) the catalyst is ineffective at lower temperatures

2 / 10

The reaction of nitrogen with hydrogen to form ammonia is exothermic. Which of these changes increases the proportion of ammonia in an equilibrium mixture of nitrogen, hydrogen and ammonia.

(i) raising the pressure at constant temperature

(ii) raising the temperature at constant pressure

(iii) decreasing the volume at constant temperature

(iv) adding a catalyst

3 / 10

What are the standard conditions for measuring standard enthalpy changes?

4 / 10

Which of the following properties increase from left to right across the series: AgCl - AgBr - AgI?

(i) intensity of colour

(ii) solubility in ammonia solution

(iii) ease of oxidation to the halogens

(iv) solubility in aqueous ammonia

5 / 10

Iodine oxidises thiosulfate ions, S2O32 -, to S4O62- . What is the oxidation number (O.N.) change for each sulfur atom?

6 / 10

The electron configuration of a chloride ion is:

7 / 10

Bubbling carbon dioxide into an aqueous solution of calcium hydroxide produces a white precipitate of:

8 / 10

What is the oxidation number of FLUORINE in

F2O

9 / 10

What is the oxidation number of SULFUR in

SO3

10 / 10

Which of these true statements help to explain why the values of the first ionisation enthalpies (energies) of the group 1 metals fall down the group from lithium to caesium?

(i) Down the group, the outer electron gets further from the nucleus

(ii) The charge on the nucleus increases down the group

(iii) Greater shielding means that the attraction between the nucleus and the outer electron reduces down the group

(iv) In all the atoms the outer electron is an s-electron

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15

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

Infra-red absorption ranges for some bonds are as follows:

C-H, 2850 - 3300 cm-1

C=C, 1620 - 1680 cm-1

C=O, 1680 - 1750 cm-1

C-O, 1000 - 1300 cm-1

O-H (alcohols), 3230 - 3550 cm-1

O-H (acids), 2500 - 3000 cm-1

The IR spectrum of propanal has one particularly strong absorption peak

This can be expected to be at:

4 / 10

The mass spectrum of copper has two significant peaks. The peak at 63 has a relative abundance of 69 and the peak at 65 has a relative abundance of 31.

This shows that the relative atomic mass of copper is:

5 / 10

Which of these pairs of compounds react to form 2-bromopropane as one of the products?

(i) prop-1-ene and hydrogen bromide at room temperature

(ii) propane and bromine in ultraviolet light

(iii) propan-2-ol on heating with sodium bromide

(iv) propan-1-ol and hydrogen bromide on heating

6 / 10

Three halogenoalkanes differ in the rate with which they react with aqueous sodium hydroxide. The order of the rates of reaction is:

7 / 10

Heating butan-1-ol with a mixture of sodium bromide and concentrated sulfuric acid produces 1-bromobutane. During the preparation the reaction mixture turns orange due to the formation of:

8 / 10

Why is ethanol a liquid while propane is a gas? (Relative atomic masses: C = 12, H = 1, O = 16)

9 / 10

The reaction that has the greatest atom economy is:

10 / 10

What is the name for this structure:

CH3CH(CH3)CH(CH3)CH2CH3?

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Chemistry Year 12 Random Retrieval

51

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

Burning a hydrocarbon fuel such as methane gas in a limited supply of air is dangerous because under these conditions one of the products is:

2 / 10

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

3 / 10

What is the mechanism for the reaction of bromine with prop-1-ene?

4 / 10

Adding a compound X, C4H10O, drop by drop to a hot acidic solution of potassium dichromate(VI) and allowing the product to distil off as it forms, produces a compound which gives a silver mirror with Tollens solution. This shows that X could be:

(i) CH3CH2CH2CH2OH

(ii)CH3CH2CHOHCH3

(iii)CH3CH(CH3)CH2OH

(iv) CH3CH2OCH2CH3

5 / 10

6 / 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

7 / 10

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

8 / 10

When chlorine reacts with cold, aqueous sodium hydroxide the ions formed are:

9 / 10

What is the mass of 0.00400 mol of sodium hydrogensulfate?

10 / 10

What is the bond angle found in BF3?

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Chemistry Year 13 Random Retrieval

26

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

Which of the following molecules is/are examples of 2o amines?

(i) 

(ii)

(iii) 

(iv) 

2 / 10

Which of these polymers would you expect to have the strongest intermolecular (interchain) forces as a result of the presence of polar covalent bonds?

3 / 10

The reaction of hydrogen gas with nitrogen monoxide gas is first order with respect to H2(g) and second order with respect to NO(g). It follows that:

(i) rate = k[H2(g)][NO(g)]2

(ii) doubling the concentration of NO(g) increases the rate by a factor of 4

(iii) the overall order of reaction is 3

(iv) halving the concentration of hydrogen reduces the rate by a factor of 1.

4 / 10

What is the value of the rate constant, k for this reaction at this temperature?

5 / 10

Consider the following equilibrium for the Haber-Bosch process:

3H2(g) + N2(g) <=>2NH3(g)

32.0 mol of H2 was combined with 12.0 mol of N2 and the mixture sealed and pressurised in a vessel of volume 2.00 dm3. The mixture was left until no further observable change in composition took place. At this point, 4.00 mol of NH3 was found to be present in the mixture. The pressure was recorded as 200 000 kPa.

Calculate the value of Kc (in units: mol-2 dm6) under these conditions.

6 / 10

Look at the chemical equation below.

2NaHCO3(s)=> Na2CO3(s)+ H2O(g)+ CO2(g)

Calculate the temperature at which this process becomes feasible.

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

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 metal forms a reddish oxide in the +1 state which dissolves in dilute sulfuric acid to give a blue solution and a red-brown precipitate?

9 / 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

10 / 10

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

BrO3- + H+ + e- => Br- + H2O

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Foundations in Chemistry Random Retrieval

17

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

Dilute hydrochloric acid reacts with:

(i) zinc to form zinc chloride and hydrogen

(ii) copper(II) oxide to form copper(II) chloride and water

(iii) zinc carbonate to form zinc chloride, carbon dioxide and water

(iv) copper to form copper(II) chloride and hydrogen

3 / 10

Which of these reactions is an acid-base reaction?

4 / 10

Which of these molecules are overall non-polar?

(i) H2O

(ii) CO2

(iii) SO2

(iv) CCl4

5 / 10

Which of these sets of properties is that of a substance which is molecular?

6 / 10

During the electrolysis of molten sodium chloride:

(i) sodium metal forms at the negative electrode

(ii) sodium ions are reduced at the cathode

(iii) chloride ions lose electrons at the positive electrode

(iv) chlorine atoms are given off as a gas at the anode

7 / 10

8 / 10

Sodium hydride reacts with water:

NaH(s) + H2O(l) -> NaOH(aq) + H2(g)

What is the concentration of a solution of sodium hydroxide formed when 0.600 g sodium hydride reacts with water and the solution is diluted to 100 cm3?

9 / 10

How many complete sub-shells are there in the phosphorus atom?

10 / 10

What is the electronic configuration of carbon?

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.

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