Problem: Nitrosyl chloride, NOCl, decomposes to NO and Cl2.2NOCl(g) ⟶ 2NO(g) + Cl2 (g)Determine the rate equation, the rate constant, and the overall order for this reaction from the following data:

🤓 Based on our data, we think this question is relevant for Professor Combrink's class at TAMIU.

FREE Expert Solution

Determine the rate equation, the rate constant, and the overall order for this reaction 


2NOCl(g) ⟶ 2NO(g) + Cl2 (g)


Step 1. Calculate the order

rate2rate1 = [NOCl]x of rate2[NOCl]x of rate18.0 × 10-103.2 × 10-9 = 0.20x[0.10]x4 = [2]x

2 raised to 2 = 4

x = 2 → 2nd order

Since there is only 1 reactant, the overall order is 2nd order


Step 2. Setup rate law

The rate law of the reaction is: rate =k[NOCl]2


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Problem Details

Nitrosyl chloride, NOCl, decomposes to NO and Cl2.

2NOCl(g) ⟶ 2NO(g) + Cl2 (g)

Determine the rate equation, the rate constant, and the overall order for this reaction from the following data:

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