Consider the reaction: h2(g) + br2(g) ⇄ 2 hbr(g) k = 81.4 at 385 °c if [h2] = [br2] = [hbr] = 0.024 m. which of the following statements is correct? the reaction proceeds towards the product, because q is greater than k the reaction proceeds towards the reactants, because q is less than k the reaction proceeds towards the product, because q is less than k the reaction is at equilibrium because the concentrations of reactants and products are equal the reaction proceeds towards the reactants, because q is greater than k

The reaction proceeds towards the product, because Q is less than K

Explanation:

We must find out the value of Q to compare with K.

H2(g) + Br2(g) ⇄ 2 HBr(g)

Q =  ([HBr]² ) / [H2] . [Br2]

If all the concentrations are the same, Q = 1.

So K > Q

The reaction proceeds towards the product, because Q is less than K

We still have reagents that have to be made into products

Q = K ---> equilibrium

Q > K > The reaction proceeds towards the reactants

Q < K > The reaction proceeds towards the product

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explanation: