Equilibrium constant with respect to concentrations of reactants and products `(K_(c))` for reaction aA+bB `harr` cC+dD where [A],[B],[C],[D] are concentrations of reactants and products

When the equilibrium is attained, the concentration of each of the reactants and products becomes equal.

which of the following is/are correct? (A) At equilibrium the concentration of reactants and product are equal (B) K_(P) = K_(C)(RT)^(Delta n) (C) When the concentration of reactants is doubled the value of equilibrium constant is also doubled (D) A catalyst doesn't alter the position of the equilibrium

A : Increasing the concentration of H_2 will increases magnitude of equilibrium constant of the reaction H_2 +I_2 hArr 2HI R: Value of K_c depends upon the concentration of reactants and products taken.

For the reaction: A + B + Q hArr C + D , if the temperature is increased, then concentration of the products will

Assertion (A) : Greater the value of K, more is the fraction of initial concentration of reactants converted to products at equilibrium. Reason (R) : The value of K depends on the initial concentration of reactants.

What is the relation between K_p and K_c for a general reaction, aA+bB iff cC+dD ?

Consider the reaction A to B . The concentration of both the reactants and the products varies exponentially with time. Which of the following figure correctly describes the change in concentration of reactants and products with time ?