Question

For the reaction below, initially the partial pressure of all 3 gases is 1.0atm. . 2NH3(g)--> N2(g) + 3H2(g) K, 0.83 1. When the reaction reach equilibrium the partial pressure of N2 will be greater than 1atm The reaction would shift toward the reactants The reaction would shift toward the products 2. When the reaction reach equilibrium the partial pressure of NH3 will be greater than 1atm 3. When the reaction reach equilibrium the partial pressure of H2 will be greater than 1atm

Answer 1

The reaction would shift toward the reactants

When the reaction reach equilibrium the partial pressure of NH3 will be greater than 1atm

Step-by-step explanation:

For the reaction:

2NH₃(g) ⇄ N₂(g) + 3H₂(g)

Where K is defined as:

`K = \frac{P_{N_(2)}*P_(H_2)^3}{P_(NH_3)^2} = 0.83`

As initial pressures of all 3 gases is 1.0atm, reaction quotient, Q, is:

`Q = \frac{1atm*{1atm}^3}{1atm^2} = 1`

As Q > K, the reaction will produce more NH₃ until Q = K consuming N₂ and H₂.

Thus, there are true:

The reaction would shift toward the reactants

When the reaction reach equilibrium the partial pressure of NH3 will be greater than 1atm