Question

) Given: CS2(g) + 3 Cl2() <= > CCl4 (8) + S2Cl2 (8) AH = -238 kJ Using arrows predict which way the equilibrium will shift ("---->" to products, <---"to reactants, or "no change") AND what will happen to the value of keq ("incr decrease", or "stays same"). Given the following perturbations: DIRECTION OF SHIFT Value of Keq ) A halving of the volume b) Adding Ne gas to the vessel -) Removing some CCIA 3) Lowering the temperature_ e) Adding some S2Cl2 O ot 625

Answer 1

These all questions can be answered by using Le Chatelier principle that is if a system in equilibrium is subjected to a change of concentration , temperature or pressure the equilibrium will shift in the direction to counterbalance the effect of the change .

1. halving the volume will shift the reaction to the forward direction that is towards the product. this could be answered using le chatliers principle , if the volume of the gaseous reaction is decreased the peressure exerted by the molecule will increase and the reaction will proceed in the direction in which this effect will decrease and as we can see from the reactions the number of gaseous molecules are greater in reactant thus they will have greater pressure thus the reaction will proceed in forward direction.

Keq is the ratio of the concentration of products to that of reactants . thus Keq will increase as the reaction will proceed in forward direction thus increasing the concentration of products.

2. adding Ne to the vessel will shift the equilibrium towards the reactants that is in backward direction at constant pressure that is towards the side with larger number of moles of gas and there is no change observed if inert gas is added at constant volume hence the equilibrium comstant Keq will decrease as the concentration of reactants increases

3.removing some CCl4 will shift the equilibrium towards the product that is in forward direction this could be explained based on le chatliers principle. Hence the Keq will increase as the concentration of product increases anf that of reactants decreases.

4. Decreasing the temperature will shift the equilibrium towards the products that is in forward direction as the reaction is exothermic as the value of △H is negative so if we decrease the temperature the reaction will proceed in forward direction in order to increase the temperature as heat is released in an exothermic reaction and hence Keq will increase .

5. adding some S2Cl2 will shift the equilibrium towards the reactants that is in backward direction this could be explained by Le chatliers principle and hence the Keq will decrease as the reactant concentration increases

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