Answer
If we reverse a chemical reaction equation the equilibrium constant becomes inverted.
If we multiply the coefficient in the reaction by a factor,then value of equilibrium constant is raised by the same factor.
Work Step by Step
Equilibrium constant ,for a chemical reaction present in equilibrium,is expressed by the concentrations of products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients which is written by law of mass action.
Consider a chemical reaction and we write equilibrium constant expression-
$A(g)+B(g)=C(g)+D(g)$
$K_{forward}=\frac{[C][D]}{[A][B]}$
Now for reverse reaction equation-
$C(g)+D(g)=A(g)+B(g$
$K_{backward}=\frac{[A][B]}{[C][D]}$
$K_{backward}=\frac{1}{\frac{[C][D]}{[A][B]}}$
$K_{backward}=\frac{1}{K_{forward}}$
So if we reverse a chemical reaction equation the equilibrium constant becomes inverted.
Rewrite the above forward reaction equation by multiplying with a factor n –
$nA(g) + nB(g) = nC(g) + nD(g)$
$K_{final}=\frac{[C]^{n}[D]^{n}}{[A]^{n}[B]^{n}}$
$K_{final}=(\frac{[C][D]}{[A][B]})^{n}$
$K_{final}=(K_{forward)})^{n}$
So if we multiply the coefficient in the reaction by a factor,then value of equilibrium constant is raised by the same factor.
