Question

For the following questions, consider the following reaction at a certain temperature: S2Cl2(g)+Cl2(g)⇌2SCl2(g) The reaction was allowed to establish equilibrium and then the equilibrium concentrations of reactants and products in the reaction mixture were measured, and recorded in the table below. (Even though this a gaseous reaction, instead of recording pressures, the concentrations of the gases were measured in molarity, making this a Kc problem. S2Cl2(g)0.050 MCl2(g)0.050 MSCl2(g)0.100 M

Part G Because the concentrations provided above are equilibrium concentrations, plug these values into the equilibrium constant expression for this balanced reaction. What is the equilibrium constant for this reaction? Before you begin, it helps to write out the equilibrium constant expression in terms of the reactants and products, then plug in the equilibrium values provided above.

Answer : Kc =  

Part H The equilibrium was then stressed by removing some Cl2 (g) involving a reaction with Na metal. Calculate the reaction quotient, Qc, if the new concentration of Cl2 = 0.030 M. Before you begin, it helps to write out the reaction quotient expression in terms of the reactants and products, then plug in the non- equilibrium values provided.

Answer: Qc =

Part I Is the value of Qc less than or greater than Kc?

A) Greater

B) Less

Part J Based on the previous question, will the reaction shift toward reactants or products to reestablish equilibrium?

A)Product

B)Reactant

Part K How does the new equilibrium concentration of S2Cl2 compare to its concentration before Cl2 was removed?

A) Lower

B)Higher

C)The same

Answer 1

Equilibrium constant Kc is defined as the ratio of concentration of product each raised to the power of their stoichiometric coefficient to the concentration of reactant each raised to the power of their stoichiometric coefficient at equilibrium. But ,

Reaction quotient Qc is defined as the ratio of concentration of product each raised to the power of their stoichiometric coefficient to the concentration of product each raised to the power of their stoichiometric coefficient at any time of reaction .

Le Chatelier principle - This principle states that if the reaction at equilibrium is subjected to the change in concentration , pressure or temperature then the equilibrium will shift in the direction which tends to counterbalance the effect of change imposed.