For the reaction $4KClO_3 \to 3KClO_4 + KCl$,if $-d[KClO_3]/dt = K_1[KClO_3]^4$,$d[KClO_4]/dt = K_2[KClO_3]^4$,and $d[KCl]/dt = K_3[KClO_3]^4$,then:
- A$K_1 = K_2 = K_3$
- B$4K_1 = 3K_2 = 2K_3$
- C$3K_1 = 4K_2 = 12K_3$
- D$K_1 = 4K_2 = 3K_3$
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For the reaction,$N_{2(g)} + 3 H_{2(g)} \longrightarrow 2 NH_{3(g)}$,$NH_{3}$ is formed at a rate of $0.088 \ mol \ dm^{-3} \ s^{-1}$. Calculate the consumption rate of $N_{2(g)}$.
If the instantaneous rate of reaction is given as $-\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$,then the reaction is represented as:
For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of disappearance of $N_{2(g)}$ is $2.22 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$. What is the rate of appearance of $NH_{3(g)}$?
For the reaction $CH_3COOCH_3 + H_2O \xrightarrow{H^{+}} CH_3COOH + CH_3OH$,the progress of the reaction is followed by:
Easy
View SolutionThermal decomposition of $N_2O_5$ occurs as per the equation below:
$2N_2O_5 \longrightarrow 4NO_2 + O_2$
The correct statement is:
$2N_2O_5 \longrightarrow 4NO_2 + O_2$
The correct statement is:
DifficultKVPY 2019
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