Which one of the following statements regarding the order of a reaction is not correct?
- AOrder can be determined experimentally.
- BOrder of reaction is equal to the sum of the powers of concentration terms in the differential rate law.
- CIt is not affected by the stoichiometric coefficients of the reactants.
- DOrder cannot be fractional.
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Similar Questions
The rate law of the reaction $2N_2O_5 \to 4NO_2 + O_2$ is
Easy
View SolutionFor a chemical reaction,the rate law is $\text{rate} = k[A]^2[B]$. If $[A]$ is doubled at constant $[B]$,the rate of reaction:
The reaction $CH_{3}COF + H_{2}O \rightleftharpoons CH_{3}COOH + HF$ is studied under two conditions:
Condition $I$: $[H_{2}O]_{0} = 1.00 \ M$,$[CH_{3}COF]_{0} = 0.01 \ M$
Condition $II$: $[H_{2}O]_{0} = 0.02 \ M$,$[CH_{3}COF]_{0} = 0.80 \ M$
Time $(t)$ min (Condition $I$) / $[CH_{3}COF]$ $M$ Time $(t)$ min (Condition $II$) / $[H_{2}O]$ $M$ $0$ / $0.01000$ $0$ / $0.0200$ $10$ / $0.00867$ $10$ / $0.0176$ $20$ / $0.00735$ $20$ / $0.0156$ $40$ / $0.00540$ $40$ / $0.0122$
Determine the overall order of the reaction and calculate the rate constant.
Condition $I$: $[H_{2}O]_{0} = 1.00 \ M$,$[CH_{3}COF]_{0} = 0.01 \ M$
Condition $II$: $[H_{2}O]_{0} = 0.02 \ M$,$[CH_{3}COF]_{0} = 0.80 \ M$
| Time $(t)$ min (Condition $I$) / $[CH_{3}COF]$ $M$ | Time $(t)$ min (Condition $II$) / $[H_{2}O]$ $M$ |
|---|---|
| $0$ / $0.01000$ | $0$ / $0.0200$ |
| $10$ / $0.00867$ | $10$ / $0.0176$ |
| $20$ / $0.00735$ | $20$ / $0.0156$ |
| $40$ / $0.00540$ | $40$ / $0.0122$ |
Determine the overall order of the reaction and calculate the rate constant.
The diazonium salt decomposes as $C_6H_5N_2^+Cl^- \to C_6H_5Cl + N_2$. At $0 \ ^\circ C$,the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Therefore,it is:
Easy
View SolutionThe mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is:
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