Which of the following statements is false ?
Which of the following statements is false ?
- A
For an endothermic reaction, energy of product is greater than that of reactant
- B
The rate law for a reaction depends on the concentrations of all reactant that appear in the stoichiometric equation.
- C
The rate of a zero order reaction is independent of the concentration of the catalyst.
- D
The specific rate constant for a reaction is independent of the concentrations of the reacting species
Similar Questions
For a certain reaction, the rate $=k[A]^2[B]$, when the initial concentration of $A$ is tripled keeping concentration of $B$ constant, the initial rate would
For a certain reaction, the rate $=k[A]^2[B]$, when the initial concentration of $A$ is tripled keeping concentration of $B$ constant, the initial rate would
- [NEET 2023]
In a reaction, $A + B \rightarrow$ product, rate is doubled when the concentration of $B$ is doubled, and rate increases by a factor of $8$ when the concentration of both the reactants $(A$ and $B)$ are doubled, rate law for the reaction can be written as
In a reaction, $A + B \rightarrow$ product, rate is doubled when the concentration of $B$ is doubled, and rate increases by a factor of $8$ when the concentration of both the reactants $(A$ and $B)$ are doubled, rate law for the reaction can be written as
- [AIPMT 2012]
Calculate the order of the reaction in $A$ and $B$
$A$
$(mol/l)$
$B$
$(mol/l)$
Rate
$0.05$
$0.05$
$1.2\times 10^{-3}$
$0.10$
$0.05$
$2.4\times 10^{-3}$
$0.05$
$0.10$
$1.2\times 10^{-3}$
Calculate the order of the reaction in $A$ and $B$
|
$A$ $(mol/l)$ |
$B$ $(mol/l)$ |
Rate |
| $0.05$ | $0.05$ | $1.2\times 10^{-3}$ |
| $0.10$ | $0.05$ | $2.4\times 10^{-3}$ |
| $0.05$ | $0.10$ | $1.2\times 10^{-3}$ |
The given reaction $2NO + {O_2} \to 2N{O_2}$ is an example of
The given reaction $2NO + {O_2} \to 2N{O_2}$ is an example of
- [AIPMT 2001]
The reaction $CH _{3} COF + H _{2} O \quad \rightleftharpoons CH _{3} COOH + HF$
Condition $I$ $:$ $\left[ H _{2} O \right]_{0}=1.00 \,M$
$\left[ CH _{3} COF \right]_{0}=0.01 \,M$
Condition $II$ $:$ $\left[ H _{2} O \right]_{0}=0.02 \,M$
$\left[ CH _{3} COF \right]_{0}=0.80 \,M$
Condition - $I$
Condition - $II$
Time
$(t)$
$min$
$\left[ CH _{3} COF \right]$ $M$
Time
$(t)$
$min$
$\left[ H _{2} O \right] \,M$
$0$
$0.01000$
$0$
$0.0200$
$10$
$0.00867$
$10$
$0.0176$
$20$
$0.00735$
$20$
$0.0156$
$40$
$0.00540$
$40$
$0.0122$
Determine the order of reaction and calculate rate constant.
The reaction $CH _{3} COF + H _{2} O \quad \rightleftharpoons CH _{3} COOH + HF$
Condition $I$ $:$ $\left[ H _{2} O \right]_{0}=1.00 \,M$
$\left[ CH _{3} COF \right]_{0}=0.01 \,M$
Condition $II$ $:$ $\left[ H _{2} O \right]_{0}=0.02 \,M$
$\left[ CH _{3} COF \right]_{0}=0.80 \,M$
| Condition - $I$ | Condition - $II$ | ||
|
Time $min$ |
$\left[ CH _{3} COF \right]$ $M$ |
Time $min$ |
$\left[ H _{2} O \right] \,M$ |
| $0$ | $0.01000$ | $0$ | $0.0200$ |
| $10$ | $0.00867$ | $10$ | $0.0176$ |
| $20$ | $0.00735$ | $20$ | $0.0156$ |
| $40$ | $0.00540$ | $40$ | $0.0122$ |
Determine the order of reaction and calculate rate constant.