GA33CHE11 - Equilibria, Acids and Bases - Science Assignment Help

Assignment Task

Answer all the questions in the spaces provided

1.1 (a) N2(g)+O2(g)2NO (g)?H298 = + 180 kJ mol-1
From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by:
Increasing the concentration of NO
Increasing the pressure
Increasing the temperature
Increasing the concentration of N2
Adding a catalyst

1.1 (b) 20739103556000N2 (g)+3H2 (g)2NH3 (g)DH is negative
From the given reaction at equilibrium above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by:
Increasing the concentration of ammonia
Increasing the pressure
Increasing the temperature
Adding a catalyst
Increasing the concentration of hydrogen will shift the equilibrium position to the left
1691005119711001.2

2(i) In the contact process: ?H = -197 kJ mol-1
Predict the position of equilibrium when:
(a) both the temperature and pressure are decreased
(b) the temperature is increased and the pressure is decreased
(ii) Explain the reasoning for using compromise temperature and pressure in industrial processes

3 (i) In the Haber process for the production of ammonia the following reaction occurs:
1994535381000N2 (g)+3H2 (g)2NH3 (g)DH is negative
If the equilibrium concentrations for all the reactants and products at 6000C are:
[N2] = 0.40 mol/dm3, [H2] = 1.20 mol/dm3 and [NH3] = 0.20 mol/ dm3
what is the numerical value of the equilibrium constant, Kc?

(ii) At 5000C Kc = 0.062 mol-2dm6. Compare this value to the one you calculated in 3(ii) above and state whether the yield of ammonia is greater at 5000C or 6000C and briefly explain your choice.

4 (a) Calculate the value of Kc for the reaction:
5008227435000PCl5 (g) PCl3 (g) +Cl2 (g) ?H = Positive
Given that when 8.4 mol of PCl5 (g) is mixed with 1.8 mol of PCl3 (g) and allowed to come to equilibrium in a 10 dm3 container the amount of PCl5 (g) at equilibrium is 7.2 mol.
Kc =
(b) Explain the effect of the following changes below on the value of Kc:
Increasing temperature
Lowering the concentration of chlorine (Cl2)
Addition of a catalyst

5 (a) Define an acid and a base according to Bronsted-Lowry
An acid is:
A base is:
(b) Explain the difference between: a strong acid or base and a weak acid or base

6. (i) Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a strong acid:
HClaq àH+aq+Cl-aq
And convert the following expression to deduce the hydrogen ion concentration:
pH = -log10 [H+]
(ii) Use the above expression to deduce the pH of HCl (aq) given the concentration of the acid to be 4.5 mol/dm3
pH =

7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case:
ethanoic acid (CH3COOH)
ammonia (NH3)
Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.

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