Question

Indicate any changes that a -d will cause for the following reaction initially at equilibrium:

C2H4(g) + Cl2(g) reverse arrows C2H4 Cl2(g) + heat

All 4 questions have the same answers

1-the system shifts in the direction of the reactants

2- the system shifts in the direction of the products

3- the equilibrium position does not change

Part A- raise the temperature of the reaction

Part B- decrease the volume of the reaction container

Part C- add a catalyst

Part D- add more Cl2(g)

Answer 1

Part A - raise the temperature of the reaction

The reaction given above is an example of an exothermic reaction, therefore, increasing the temperature will shift the reaction in the backward direction. thus equilibrium will shift in the direction of the reactants. thus point 1 is correct.

Part B - decrease the volume of the reaction container

Decreasing the volume of the container shifts the equilibrium to the side with fewest moles of gas. In the reaction given above the product side is having one mole of gas, therefore, the reaction shifts in the direction of the products. Thus point 2 is correct

Part C - add a catalyst

Addition of a catalyst does not shift the position of the equilibrium, therefore answer is point 3.

Part D - add more Cl2(g)

Addition of reactant shifts the reaction towards product thus the answer is point 2.