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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

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Answer:

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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