Question

General chemical reaction equation in which reactants A and B react to give product C and D is given as :
$aA+bB⟶cC+dD$
The mass action law states that if the system is at equilibrium at a given temperature, then the following ratio is a constant. Which is that ratio among the following ?

• A. $\frac{\left[C{]}^c\right[D{]}^d}{\left[A{]}^a\right[B{]}^b}$
• B. $\frac{\left[C{]}^a\right[D{]}^b}{\left[A{]}^c\right[B{]}^d}$
• C. $\frac{\left[C{]}^d\right[D{]}^a}{\left[A{]}^b\right[B{]}^a}$
• D. $\frac{\left[C\right]\left[D\right]}{\left[A\right]\left[B\right]}$

Answer 1

The correct option is A $\frac{\left[C{]}^c\right[D{]}^d}{\left[A{]}^a\right[B{]}^b}$

The mass action law states that if the system is at equilibrium at a given temperature, then the following ratio is a constant.
$\frac{\left[C{]}^c\right[D{]}^d}{\left[A{]}^a\right[B{]}^b}$.
This ratio is called the equilibrium constant K.