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

the answer

explanation:

the capillary tube was too close to the bottom of the beaker.

the ruler may have moved.

water got into the capillary tube.

the temperature was not allowed to equilibrate in the 2-4 minutes.