The rate constant for the reaction, $2{N_2}{O_5} \to 4N{O_2}$ $ + {O_2}$ is $3 \times {10^{ - 5}}{\sec ^{ - 1}}$. If the rate is $2.40 \times {10^{ - 5}}\,mol\,\,litr{e^{{\rm{ - 1}}}}{\sec ^{ - 1}}$. Then the concentration of ${N_2}{O_5}$ (in mol litre $^{-1}$) is
The rate constant for the reaction, $2{N_2}{O_5} \to 4N{O_2}$ $ + {O_2}$ is $3 \times {10^{ - 5}}{\sec ^{ - 1}}$. If the rate is $2.40 \times {10^{ - 5}}\,mol\,\,litr{e^{{\rm{ - 1}}}}{\sec ^{ - 1}}$. Then the concentration of ${N_2}{O_5}$ (in mol litre $^{-1}$) is
- [IIT 2000]
- A
$1.4$
- B
$1.2$
- C
$0.04$
- D
$0.8$
Similar Questions
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then
In the reaction, $A + B \to C + D$ , the rate $\left( {\frac{{dx}}{{dt}}} \right)$ when plotted against time $'t'$ gives a straight line parallel to time axis. The order and rate of reaction will be
In the reaction, $A + B \to C + D$ , the rate $\left( {\frac{{dx}}{{dt}}} \right)$ when plotted against time $'t'$ gives a straight line parallel to time axis. The order and rate of reaction will be
The following mechanism has been proposed for the reaction of $NO$ with $Br_2$ to form $NOBr$ :
$NO(g) + Br_2 (g) \rightleftharpoons NOBr_2 (g)$
$NOBr_2(g)+ NO(g) \longrightarrow 2NOBr(g)$
If the second step is the rate determining step, the order of the reaction with respect to $NO(g)$ is
The following mechanism has been proposed for the reaction of $NO$ with $Br_2$ to form $NOBr$ :
$NO(g) + Br_2 (g) \rightleftharpoons NOBr_2 (g)$
$NOBr_2(g)+ NO(g) \longrightarrow 2NOBr(g)$
If the second step is the rate determining step, the order of the reaction with respect to $NO(g)$ is
- [AIEEE 2006]
The rate of certain reaction depends on concentration according to the equation $\frac{{ - dc}}{{dt}} = \frac{{{K_1}C}}{{1 + {K_2}C}},$ what is the order, when concentration $(c)$ is very-very high
The rate of certain reaction depends on concentration according to the equation $\frac{{ - dc}}{{dt}} = \frac{{{K_1}C}}{{1 + {K_2}C}},$ what is the order, when concentration $(c)$ is very-very high
Reaction $aA + bB\,\to $ product. The rate of reaction $= k[A]^3\, [B]^0$ if the concentration of $A$ is double and concentration of $B$ is half the rate will be ?
Reaction $aA + bB\,\to $ product. The rate of reaction $= k[A]^3\, [B]^0$ if the concentration of $A$ is double and concentration of $B$ is half the rate will be ?