Question

Express the equilibrium constant for the following reaction.P4O10(s) ↔ P4(s) + 5 O2(g)K = [P4][O2]^5/[P4O10]K = [O2]^5K = [P4O10]/[P4][O2]^1/5K = [O2]^-5K = [P4O10]/[P4][O2]^5

Answer 1

The equilibrium constant (K) for the given reaction can be expressed as [P4][O2]^5/[P4O10]. This expression represents the ratio of the concentrations of the products raised to their respective coefficients, divided by the concentration of the reactant. The value of K can be calculated based on the given concentrations.

Step-by-step explanation:

The equilibrium constant (K) for the given reaction can be expressed as:

K = [P4][O2]^5/[P4O10]

This expression represents the ratio of the concentrations of the products (P4 and O2) raised to their respective coefficients, divided by the concentration of the reactant (P4O10).

For example, if the concentration of P4 is 0.1 M, the concentration of O2 is 0.2 M, and the concentration of P4O10 is 0.05 M, the value of K can be calculated as:

K = (0.1 * (0.2)^5) / 0.05 = 0.64

Answer 2

Answer : The correct expression for equilibrium constant will be,
`K=[O_2]^5`

Explanation :

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.

As we know that the concentrations of pure solids are constant that is they do not change. Thus, they are not included in the equilibrium expression.

The given equilibrium reaction is,

`P_4O_(10)(s)\rightleftharpoons P_4(s)+5O_2(g)`

The expression of
`K` will be,

`K=[O_2]^5`

Therefore, the correct expression for equilibrium constant will be,
`K=[O_2]^5`