At 473 K, for the reversible elementary reaction k 1=7.8×102 M-1 s-1 and k 1=4.7

Question

At 473 K, for the reversible elementary reaction

k1=7.8×102 M-1 s-1 and k1=4.7×102 M-2 s-1. A sample of NOCl is placed in a container and heated to 473 K. When the system comes to equilibrium, [NOCl] is found to be 0.11 mol/L .What is the equilibrium concentration of [NO]?

Hint: Equilibrium is achieved when the forward reaction rate is equal to the reverse reaction rate.

[NO] = ___ M

please explain using the ice table

that really help me understand and do well on exam

please fully explain step by step.

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Explanation / Answer

Rate of forward reaction, rf = k1[NOCl]2

Rate of backward reaction , rb = k-1[NO]2[Cl2]

At equilibrium, rate of forward reaction = rate of backward reaction

rf = rb

k1[NOCl]2 = k-1[NO]2[Cl2]

k1/k-1 = [NOCl]2/[NO]2[Cl2]

K = [NOCl]2/[NO]2[Cl2]

where, K = k1/k-1 = 7.8 * 10-2 / 4.7*102 = 1.6 * 10-4

And at equilibrium, [NO] = [Cl2] = x

so, 1.6 * 10-4 = (0.11)2 / (x)2(x)

X3 = 0.012 / (1.6*10-4)

x = (75.)(1/3)

x = 4.2 M

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