Question

Statement: The equilibrium mole obtained during the experiment for the given reaction in 1 L vessel is shown below the reactants and products.
$2A\left(g\right)+B\left(g\right)\rightleftharpoons 3C\left(g\right)+3D$
At equilibrium: 8 mol 16 mol 4 mol 4 mol

If the reaction in the forward direction is to be made, the initial concentration of reactants and products should be such that the reaction quotient should be less than four.

If the given statement is true enter 1 if false enter 0.

Answer 1

The value of the equilibrium constant K is as calculated below.

$K=\frac{\left[C{]}^3\right[D{]}^3}{\left[A{]}^2\right[B]}=\frac{4^3\times 4^3}{8^2\times 16}=4$.

If the reaction in the forward direction is to be made, the initial concentration of reactants and products should be such that reaction quotient should be less than four. This will ensure that more reactants and lesser products are present in the reaction mixture which will derive the equilibrium in the forward direction.

Hence, the given statement is $true$ and the correct entry is $1$