Physical Chemistry & Transition Elements Random Retrieval

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 Br_2(aq) oxidise Cr³⁺_(aq) to dichromate(VI)?

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

Look at the chemical equation below.

CH_4(g) + H₂O_(g)=> CO_(g)+ 3H_2(g)

Using your answers to Questions 6 and 7, calculate the Gibbs Energy change ΔG, for the process if it is carried out in a reactor vessel at 1500^oC.

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

Calculate the value of the enthalpy change associated with the following equation?

2Cl_2(g)=> 4Cl_(g)

What enthalpy change is represented by the following equation?

½ Br_2(l) => Br_(g)

Consider the following equilibrium:

3Fe_(s) + 4H₂O_(g) <=>Fe₃O_4(s)+ 4H_2(g)

40.0 g of iron wool was placed in a vessel of volume 2.00 dm³. The iron was exposed to 20.0 mol of high pressure steam and the system allowed to settle to equilibrium. At equilibrium, 0.250 mol of hydrogen was found in the vessel. The gauge on the pressure vessel read 1 000 kPa. The volume of iron wool was insignificant.

Calculate the value of K_c (no units) under these conditions.

These reactions are rapid at 298 K. Which of the reactions goes effectively to completion?

(i) I^-_(aq) + I_2(aq) <=> I₃^-_(aq) K_c = 7.1 x 10^-2 mol^-1 dm³

(ii) Cu²⁺_(aq) + 4NH_3(aq) <=> [Cu(NH₃)₄]²⁺_(aq) K_c = 1.4 x 10¹³ mol^-4dm¹²

(iii) 2H₂O_(l) <=> H₃O⁺_(aq) + OH^-_(aq) K_c = 1.0 x 10^-14 mol² dm^-6

(iv) Cu²⁺_(aq) + Zn_(s) <=> Cu_(s) + Zn²⁺_(aq) K_c = 1 x 10³⁷

For the equilibrium: CaCO_3(s) <=> CaO_(s) + CO_2(g)

Consider the synthesis of methanol in the following equilibrium:

CO_(g) + 2H_2(g) <=>CH₃OH_(g)

2.00 mol of CO was mixed with 4.00 mol of H₂ and the mixture sealed in a container. The mixture was left until no further observable change in composition took place. At this point, 1.90 mol of CH₃OH was present in the mixture.

Calculate the value of the mole fraction of CH₃OH present in the mixture under these conditions.

Consider the following equilibrium for the Haber-Bosch process:

3H_2(g) + N_2(g) <=>2NH_3(g)

6.00 mol of H₂ was combined with 6.00 mol of N₂ and the mixture sealed in a heated and pressurised vessel with an iron catalyst. The mixture was left until no further observable change in composition took place. At this point, 3.00 mol of NH₃ was found to be present in the mixture.

Calculate the value of the mole fraction of NH₃ present in the mixture under these conditions.