In the following reaction $A \longrightarrow B + C$, rate constant is $0.001\, Ms^{-1}$. If we start with $1\, M$ of $A$ then concentration of $A$ and $B$ after $10\, minutes$ are respectively
In the following reaction $A \longrightarrow B + C$, rate constant is $0.001\, Ms^{-1}$. If we start with $1\, M$ of $A$ then concentration of $A$ and $B$ after $10\, minutes$ are respectively
- A
$0.5\, M, \,\,0.5\, M$
- B
$0.6\, M,\,\, 0.4\, M$
- C
$0.4\, M,\,\, 0.6\, M$
- D
None of these
Similar Questions
The half life for the decomposition of gaseous compound $A$ is $240\,s$ when the gaseous pressure was $500\,Torr$ initially. When the pressure was $250\,Torr$, the half life was found to be $4.0\,min$. The order of the reaction is....... (Nearest integer)
The half life for the decomposition of gaseous compound $A$ is $240\,s$ when the gaseous pressure was $500\,Torr$ initially. When the pressure was $250\,Torr$, the half life was found to be $4.0\,min$. The order of the reaction is....... (Nearest integer)
- [JEE MAIN 2022]
Which of the following oxides of nitrogen will be the most stable one
Which of the following oxides of nitrogen will be the most stable one
The rate of dissappearance of $MnO_4^-$ in the following reaction is $4.56 \times 10^{-3}\, M/s$
$2MnO_4^-+ 10I^-+ 16H^+ \to 2Mn^{2+} + 5I_2 + 8 H_2O$
The rate of apperance of $I_2$ is
The rate of dissappearance of $MnO_4^-$ in the following reaction is $4.56 \times 10^{-3}\, M/s$
$2MnO_4^-+ 10I^-+ 16H^+ \to 2Mn^{2+} + 5I_2 + 8 H_2O$
The rate of apperance of $I_2$ is
For reaction a $A \to x\;P$, when $[A] = 2.2\,m\,M$, the rate was found to be $2.4\;m\,M\;{s^{ - 1}}$. On reducing concentration of $A$ to half, the rate changes to $0.6\;m\,M\;{s^{ - 1}}$. The order of reaction with respect to $A$ is
For reaction a $A \to x\;P$, when $[A] = 2.2\,m\,M$, the rate was found to be $2.4\;m\,M\;{s^{ - 1}}$. On reducing concentration of $A$ to half, the rate changes to $0.6\;m\,M\;{s^{ - 1}}$. The order of reaction with respect to $A$ is
- [AIIMS 2005]
The experimental data for reaction
$2A + B_2 \longrightarrow 2AB$
Exp.
$[A]$
$[B_2]$
Rate $(mol\,L^{-1}\,S^{-1})$
$1$
$0.50$
$0.50$
$1.6 \times {10^{ - 4}}$
$2$
$0.50$
$1.00$
$3.2 \times {10^{ - 4}}$
$3$
$1.00$
$1.00$
$3.2 \times {10^{ - 4}}$
The rate law
The experimental data for reaction
$2A + B_2 \longrightarrow 2AB$
| Exp. | $[A]$ | $[B_2]$ | Rate $(mol\,L^{-1}\,S^{-1})$ |
| $1$ | $0.50$ | $0.50$ | $1.6 \times {10^{ - 4}}$ |
| $2$ | $0.50$ | $1.00$ | $3.2 \times {10^{ - 4}}$ |
| $3$ | $1.00$ | $1.00$ | $3.2 \times {10^{ - 4}}$ |
The rate law