Which of the following statements is true?
1. the equilibrium-constant expression depends on the stoichiometry of the reaction.
2. the value of the equilibrium constant varies with temperature.
3. the value of the equilibrium constant depends on the initial amounts of the reactants and products.

Option A and B

Explanation:

The equilibrium constant expression is the ratio of the active equilibrium concentration of the products to that of reactant in which each raised to power of their stoichiometric coefficients.

Thus, option A is correct.

The equilibrium constant is only dependent on temperature. Its value increase/ decrease depending upon the forward reaction to be exothermic or endothermic.

For an exothermic reaction,

On increasing the temperature, reaction will go in backward direction (towards left), because according to Le Chatelier's principle as we increase the temperature,  the equilibrium is will be disturbed , so to again establish the equilibrium, the temperature need to be reduced , hence , the reaction will go in backward direction (towards left).

On decreasing the temperature, reaction will go in forward direction (towards right), because according to Le Chatelier's principle as we decrease the temperature,  the equilibrium is will be disturbed , so to again establish the equilibrium, the temperature need to be increased , hence , the reaction will go in forward direction (towards right).

The same is vice versa for endothermic reactions.

Hence, option B is correct.

Option C is incorrect as equilibrium constant only depends on temperature.

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.

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