For the reaction pc15 (8) pc13 (g) + cl2 (g) k = 0.0454 at 261 °c. if a vessel is filled with these gases such that the initial concentrations are [pc15) = 0.20 m, [pc13] = 0.20 m, and (cl21 = 2.5 m, in which direction will a reaction occur and why? a) toward products because qc = 0.56 b) toward reactants because qc = 2.5 c) toward products because qc = 2.8 d) toward reactants because qc = 0.0454 e) it is at equilibrium because qc = 1

The correct answer is B.

The is samller than of the reaction . So,the reaction will shift towards the left i.e. towards the reactant side.

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

The expression for is written as:

Given : = 0.0454

Thus as , the reaction will shift towards the left i.e. towards the reactant side.

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