Question

I’m stuck with this question I don’t know if I have the right steps and how to get the answer

Answer 1

Step 1

The reaction is written:

2 NOCl (g) <=> 2 NO (g) + Cl2 (g)

Step 2

2 NOCl (g) <=> 2 NO (g) + Cl2 (g)

Initial 1 mol/1 L = 1 M 0 0

When says: "it is decomposed 9.0 %" it means:

From the initial value of NOCl only is decomposed 9.0 % of 1 M, so:

0.09 x 1 M = 0.09 M

What remains is = 1 M - 0.09 = 0.91 M = this is the concentration in equilibrium for NOCl.

Now, what is formed on the right side:

For NO) +2x = 0.09 => x = 0.09/2 => x = 0.045 M

For Cl2) +x = 0.045 M

Therefore, concentrations on the right side, in equilibrium:

For NO) 0.09 M

For Cl2) 0.045 M

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Step 3