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At the start of a reaction, there are 0.0249 mol N2,
3.21 x 10-2 mol H2, and 6.42 x 10-4 mol NH3 in a
3.50 L reaction vessel at 375°C. If the equilibrium constant, K, for the reaction:
N2(g) + 3H2(g)= 2NH3(g)
is 1.2 at this temperature, decide whether the system is at equilibrium or not. If it is not, predict in which direction, the net reaction will proceed.​

Answer :

ajeigbeibraheem

Answer:

Explanation:

The reaction is given as:

[tex]N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}[/tex]

The reaction quotient is:

[tex]Q_C = \dfrac{[NH_3]^2}{[N_2][H_2]^3}[/tex]

From the given information:

TO find each entity in the reaction quotient, we have:

[tex][NH_3] = \dfrac{6.42 \times 10^{-4}}{3.5}\\ \\ NH_3 = 1.834 \times 10^{-4}[/tex]

[tex][N_2] = \dfrac{0.024 }{3.5}[/tex]

[tex][N_2] = 0.006857[/tex]

[tex][H_2] =\dfrac{3.21 \times 10^{-2}}{3.5}[/tex]

[tex][H_2] = 9.17 \times 10^{-3}[/tex]

∴

[tex]Q_c= \dfrac{(1.834 \times 10^{-4})^2}{(0.0711)\times (9.17\times 10^{-3})^3} \\ \\ Q_c = 0.6135[/tex]

However; given that:

[tex]K_c = 1.2[/tex]

By relating [tex]Q_c \ \ and \ \ K_c[/tex], we will realize that [tex]Q_c \ \ < \ \ K_c[/tex]

The reaction is said that it is not at equilibrium and for it to be at equilibrium, then the reaction needs to proceed in the forward direction.

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