Which one of the following statement for order of reaction is not correct ?
Which one of the following statement for order of reaction is not correct ?
- A
Order is determined experimentally.
- B
Order of reaction is equal to sum of powers of concentration terms in experimental rate law.
- C
It is not affected by the stoichiometric coefficient of the reactants.
- D
Order cannot be fractional.
Similar Questions
Select the correct statement
Select the correct statement
Explain order of reaction of complex reaction by giving examples.
Explain order of reaction of complex reaction by giving examples.
Rate of reaction is given by following rate law $ - \frac{{d\left[ c \right]}}{{dt}} = \frac{{{k_1}\,\left[ c \right]}}{{1 + {k_2}\,\left[ c \right]}}$ order of reaction when concentration is verh high
Rate of reaction is given by following rate law $ - \frac{{d\left[ c \right]}}{{dt}} = \frac{{{k_1}\,\left[ c \right]}}{{1 + {k_2}\,\left[ c \right]}}$ order of reaction when concentration is verh high
During the kinetic study of the reaction, $2A + B \rightarrow C + D,$ 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?
During the kinetic study of the reaction, $2A + B \rightarrow C + D,$ 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?
- [AIPMT 2010]
$A_2 + 2\,B \to 2\,AB$
$[A_2]$
$[B]$
${-d\,[A_2]/dt}$
$0.1$
$0.2$
$1 \times {10^{ - 2}}\,M{s^{ - 1}}$
$0.2$
$0.2$
$2 \times {10^{ - 2}}\,M{s^{ - 1}}$
$0.2$
$0.4$
$8 \times {10^{ - 2}}\,M{s^{ - 1}}$
Order of reaction w.r.t. $A_2$ and $B$ are respectively
$A_2 + 2\,B \to 2\,AB$
| $[A_2]$ | $[B]$ | ${-d\,[A_2]/dt}$ |
| $0.1$ | $0.2$ | $1 \times {10^{ - 2}}\,M{s^{ - 1}}$ |
| $0.2$ | $0.2$ | $2 \times {10^{ - 2}}\,M{s^{ - 1}}$ |
| $0.2$ | $0.4$ | $8 \times {10^{ - 2}}\,M{s^{ - 1}}$ |
Order of reaction w.r.t. $A_2$ and $B$ are respectively