Total order of reaction $X + Y \rightarrow XY$ is $3$. The order of reaction with respect to $X$ is $2$. State the differential rate equation for the reaction.
- A$-\frac{d[X]}{dt} = K[X]^0[Y]^3$
- B$-\frac{d[X]}{dt} = K[X]^3[Y]^0$
- C$-\frac{d[X]}{dt} = K[X]^2[Y]$
- D$-\frac{d[X]}{dt} = K[X][Y]^2$
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For a chemical reaction $Y + 2Z \to$ Product,the rate-controlling step is $Y + \frac{1}{2}Z \to Q$. If the concentration of $Z$ is doubled,the rate of reaction will:
Difficult
View SolutionThe hypothetical reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism given below. What is the overall order of the reaction?
$A_2 \rightleftharpoons A + A$ ...... (fast);
$A + B_2 \rightarrow AB + B$ ...... (slow);
$A + B \rightarrow AB$ ...... (fast)
$A_2 \rightleftharpoons A + A$ ...... (fast);
$A + B_2 \rightarrow AB + B$ ...... (slow);
$A + B \rightarrow AB$ ...... (fast)
Medium
View SolutionFill in the blanks:
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$
Difficult
View SolutionThe order of a reaction for an esterification process is . . . . . . .
At a certain temperature,the half-life periods for the catalytic decomposition of $NH_3$ were found to be as follows:
Pressure $(mm \ Hg)$ $50, 100, 200$ Half-life period $(hrs)$ $3.52, 1.76, 0.88$
What will be the pressure when the half-life period is $2.5 \ hrs$?
| Pressure $(mm \ Hg)$ | $50, 100, 200$ |
| Half-life period $(hrs)$ | $3.52, 1.76, 0.88$ |
What will be the pressure when the half-life period is $2.5 \ hrs$?
Medium
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