During the kinetic study of the reaction,$2A + B \rightarrow C + D,$ the following results were obtained:
$Run$ $[A] / mol \ L^{-1}$ $[B] / mol \ L^{-1}$ Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$ $I.$ $0.1$ $0.1$ $6.0 \times 10^{-3}$ $II.$ $0.3$ $0.2$ $7.2 \times 10^{-2}$ $III.$ $0.3$ $0.4$ $2.88 \times 10^{-1}$ $IV.$ $0.4$ $0.1$ $2.40 \times 10^{-2}$
Based on the above data,which one of the following is correct?
| $Run$ | $[A] / mol \ L^{-1}$ | $[B] / mol \ L^{-1}$ | Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$ |
| $I.$ | $0.1$ | $0.1$ | $6.0 \times 10^{-3}$ |
| $II.$ | $0.3$ | $0.2$ | $7.2 \times 10^{-2}$ |
| $III.$ | $0.3$ | $0.4$ | $2.88 \times 10^{-1}$ |
| $IV.$ | $0.4$ | $0.1$ | $2.40 \times 10^{-2}$ |
Based on the above data,which one of the following is correct?
- ARate $= k[A]^2[B]$
- BRate $= k[A][B]$
- CRate $= k[A]^2[B]^2$
- DRate $= k[A][B]^2$
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Similar Questions
The reaction of hydrogen and iodine monochloride is given as
$H_{2(g)} + 2ICl_{(g)} \to 2HCl_{(g)} + I_{2(g)}$
This reaction is of first order with respect to $H_{2(g)}$ and $ICl_{(g)}$. Which of the following mechanisms is consistent with the given information?
Mechanism $A$:
$H_{2(g)} + 2ICl_{(g)} \to 2HCl_{(g)} + I_{2(g)}$
Mechanism $B$:
$H_{2(g)} + ICl_{(g)} \to HCl_{(g)} + HI_{(g)}$ (Slow)
$HI_{(g)} + ICl_{(g)} \to HCl_{(g)} + I_{2(g)}$ (Fast)
$H_{2(g)} + 2ICl_{(g)} \to 2HCl_{(g)} + I_{2(g)}$
This reaction is of first order with respect to $H_{2(g)}$ and $ICl_{(g)}$. Which of the following mechanisms is consistent with the given information?
Mechanism $A$:
$H_{2(g)} + 2ICl_{(g)} \to 2HCl_{(g)} + I_{2(g)}$
Mechanism $B$:
$H_{2(g)} + ICl_{(g)} \to HCl_{(g)} + HI_{(g)}$ (Slow)
$HI_{(g)} + ICl_{(g)} \to HCl_{(g)} + I_{2(g)}$ (Fast)
For the inversion of cane sugar,the half-life is $500 \ min$ at all concentrations of sugar when $pH = 5$. However,when $pH = 6$,the half-life becomes $50 \ min$. Determine the rate law for the inversion of cane sugar.
Difficult
View SolutionWhich one of the following is a second order reaction?
The following data are obtained for a reaction,$X + Y \rightarrow$ Products.
$Expt.$ $[X]_0 / mol \ L^{-1}$ $[Y]_0 / mol \ L^{-1}$ $Rate / mol \ L^{-1} s^{-1}$ $1$ $0.25$ $0.25$ $1.0 \times 10^{-6}$ $2$ $0.50$ $0.25$ $4.0 \times 10^{-6}$ $3$ $0.25$ $0.50$ $8.0 \times 10^{-6}$
The overall order of the reaction is:
| $Expt.$ | $[X]_0 / mol \ L^{-1}$ | $[Y]_0 / mol \ L^{-1}$ | $Rate / mol \ L^{-1} s^{-1}$ |
| $1$ | $0.25$ | $0.25$ | $1.0 \times 10^{-6}$ |
| $2$ | $0.50$ | $0.25$ | $4.0 \times 10^{-6}$ |
| $3$ | $0.25$ | $0.50$ | $8.0 \times 10^{-6}$ |
The overall order of the reaction is:
MediumKVPY 2012
View SolutionWrite the unit of the rate constant for the following reactions:
$1.$ $5/2$ order
$2.$ $n$ order
$1.$ $5/2$ order
$2.$ $n$ order
Easy
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