ABC26PH0669 · Chemical Kinetics

Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Rate Laws Order · Exam: JAM 2001-2022 · Marks: 2 · Difficulty: Hard

For the reaction:
\[ 2 \mathrm{NO}+2 \mathrm{H}_{2} \xrightarrow{700^{\circ} \mathrm{C}} \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O} \]
(i) Write the expression for the rate of the reaction in terms of the change in concentrations of NO and $\mathrm{H}_{2} \mathrm{O}$. (ii) Given the following data for the above reaction, find the order of the reaction with respect to (a) NO and (b) $\mathrm{H}_{2}$ and the rate constant of the reaction along with the proper unit,
$[\mathrm{NO}]_{\mathrm{t}=0}\,(\mathrm{mol\,dm^{-3}})$$[\mathrm{H_2}]_{\mathrm{t}=0}\,(\mathrm{mol\,dm^{-3}})$Intial rate $(\mathrm{mol\,dm^{-3}\,s^{-1}})$
Experiment 10.0250.01$2.4 \times 10^{-6}$
Experiment 20.0250.005$1.2 \times 10^{-6}$
Experiment 30.01250.01$0.6 \times 10^{-6}$
Answer
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Explanation
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