What is the order of a reaction which has a rate expression rate $ = K{[A]^{3/2}}{[B]^{ - 1}}$
What is the order of a reaction which has a rate expression rate $ = K{[A]^{3/2}}{[B]^{ - 1}}$
- A
$3/2$
- B
$1/2$
- C
$0$
- D
None of these
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Which of the following optioms correctly represents relationship between $t_{7/8}$ and $t_{1/2}$ where $t_{7/8}$ represent time required for concentration to become $\frac{1}{8} \,th$ of original for a reaction of order $'n'$
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What is molecularity of a relation ? Explain its types by examples.
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The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
Experiment
$[ A ] / mol\, ^{-1}$
$[ B ] / mol\, ^{-1}$
Initial rate $/$ $mol$ $L^{-1}$ $min$ $^{-1}$
$I$
$0.1$
$0.1$
$2.0 \times 10^{-2}$
$II$
-
$0.2$
$4.0 \times 10^{-2}$
$III$
$0.4$
$0.4$
-
$IV$
-
$0.2$
$2.0 \times 10^{-2}$
The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
| Experiment | $[ A ] / mol\, ^{-1}$ | $[ B ] / mol\, ^{-1}$ | Initial rate $/$ $mol$ $L^{-1}$ $min$ $^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $2.0 \times 10^{-2}$ |
| $II$ | - | $0.2$ | $4.0 \times 10^{-2}$ |
| $III$ | $0.4$ | $0.4$ | - |
| $IV$ | - | $0.2$ | $2.0 \times 10^{-2}$ |
The rate law for reaction $A + 2B = C + 2D$ will be
The rate law for reaction $A + 2B = C + 2D$ will be
Consider the reaction, $2A + B \rightarrow$ products. When concentration of $B$ alone was doubled, the half-life did not change. When the concentration of $A$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is
Consider the reaction, $2A + B \rightarrow$ products. When concentration of $B$ alone was doubled, the half-life did not change. When the concentration of $A$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is
- [AIEEE 2007]