Discussion Questions 1. Given the equilibrium equation for a general reaction, A + B  C + D, explain what happens to the reactants and products from time 0 until the time at which the reaction reaches equilibrium. 2. Given this reaction at equilibrium, C (s) + CO2 (g)  2CO (g) (∆H° = 119kJ), explain the changes that would occur when the following stresses are applied or removed for this reaction. (a) CO is removed. (b) Heat is added. (c) CO2 is added. (d) Heat is removed.

Question

Niko Murphy

Chemistry

2 October, 05:15

Discussion Questions 1. Given the equilibrium equation for a general reaction, A + B  C + D, explain what happens to the reactants and products from time 0 until the time at which the reaction reaches equilibrium. 2. Given this reaction at equilibrium, C (s) + CO2 (g)  2CO (g) (∆H° = 119kJ), explain the changes that would occur when the following stresses are applied or removed for this reaction. (a) CO is removed. (b) Heat is added. (c) CO2 is added. (d) Heat is removed.

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Answers (1)

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Casey Villanueva · Answer 1

Answer:The equilibrium constant for a given reaction is [concentration of products]/[concentration of reactants].

Explanation:

Equilibrium constant=[concentration of products]/[concentration of reactants]

The concentration of reactant molecules is maximum at time 0 and it decreases as the reaction proceeds, The concentration of product molecules increases. At equilibrium the concentration of reactants and products are equal.

All the changes would occur in accordance with the LeChateliers principle.

For the given reaction the following changes would occur:

a When CO is removed from the reaction mixture so the reaction would shift towards right that is in forward direction as we are decreasing the concentration of CO so the system would try to increase the concentration of CO and that can happen by more production of CO.

b Since the above reaction is an endothermic reaction so when we would be adding heat to the system that is when we would increase the temperature the reaction would shift forwards as more heat energy is absorbed by reactants to form more products.

c When more CO₂ is added so more amount of reactants are added to the system so the system would try to decrease the amount of reactants that is CO₂ and hence more amount of products would be formed. The reaction would shift in forward direction.

d Since this reaction is endothermic in nature so when we remove the heat from reaction hence even less amount of heat is present in the system and so the reaction shift in backward direction as the reaction cannot proceed without enough amount of heat.