consider the reaction.\nn₂(g) + 3h₂(g)⇌2nh₃(g)\nat equilibrium, the concentrations of the different species…

consider the reaction.\nn₂(g) + 3h₂(g)⇌2nh₃(g)\nat equilibrium, the concentrations of the different species are as follows.\nnh₃ = 0.105 m\nn₂ = 1.1 m\nh₂ = 1.50 m\nwhat is the equilibrium constant for the reaction at this temperature?\n0.0030\n0.030\n34\n340

consider the reaction.\nn₂(g) + 3h₂(g)⇌2nh₃(g)\nat equilibrium, the concentrations of the different species are as follows.\nnh₃ = 0.105 m\nn₂ = 1.1 m\nh₂ = 1.50 m\nwhat is the equilibrium constant for the reaction at this temperature?\n0.0030\n0.030\n34\n340

Answer

Explanation:

Step1: Write equilibrium - constant expression

For the reaction $N_2(g)+3H_2(g)\rightleftharpoons2NH_3(g)$, the equilibrium - constant expression $K_c$ is given by $K_c=\frac{[NH_3]^2}{[N_2][H_2]^3}$.

Step2: Substitute the given concentrations

Substitute $[NH_3]=0.105\ M$, $[N_2]=1.1\ M$, and $[H_2]=1.50\ M$ into the expression: [ \begin{align*} K_c&=\frac{(0.105)^2}{1.1\times(1.50)^3}\ &=\frac{0.011025}{1.1\times3.375}\ &=\frac{0.011025}{3.7125}\ & = 0.0030 \end{align*} ]

Answer:

0.0030