For a reaction $\frac{1}{2} A \rightarrow 2 B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by the expression:
- A$\frac{-d[A]}{dt} = 4 \frac{d[B]}{dt}$
- B$\frac{-d[A]}{dt} = \frac{1}{4} \frac{d[B]}{dt}$
- C$\frac{-d[A]}{dt} = \frac{1}{2} \frac{d[B]}{dt}$
- D$\frac{-d[A]}{dt} = \frac{d[B]}{dt}$
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Similar Questions
Calculate the instantaneous rate $(r_{inst})$ based on the example problem $-1$ graphically for the times $250\ s$,$350\ s$,$450\ s$,and $600\ s$.
Difficult
View SolutionConsider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?
The following results are obtained in the hydrolysis of chlorobutane $(C_4H_9Cl)$:
Time $(s)$ $0$ $100$ $200$ $300$ $400$ $700$ $800$ $[C_4H_9Cl]$ $(mol \, L^{-1})$ $0.100$ $0.082$ $0.067$ $0.055$ $0.044$ $0.021$ $0.017$
Calculate the average rate $r_{av}$ of the reaction during different time intervals.
| Time $(s)$ | $0$ | $100$ | $200$ | $300$ | $400$ | $700$ | $800$ |
| $[C_4H_9Cl]$ $(mol \, L^{-1})$ | $0.100$ | $0.082$ | $0.067$ | $0.055$ | $0.044$ | $0.021$ | $0.017$ |
Calculate the average rate $r_{av}$ of the reaction during different time intervals.
Medium
View SolutionIn the reaction,$N_{2} + 3H_{2} \longrightarrow 2NH_{3}$,the rate of disappearance of $H_{2}$ is $0.02 \ M/s$. The rate of appearance of $NH_{3}$ is (in $M/s$)
$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:
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