Which of the following is an example of a first-order reaction?
- A$2 NH_{3(g)} \rightarrow N_{2(g)} + 3 H_{2(g)}$
- B$2 H_2 O_{2(aq)} \rightarrow 2 H_2 O_{(l)} + O_{2(g)}$
- C$4 PH_{3(g)} \xrightarrow{W} P_{4(g)} + 6 H_{2(g)}$
- D$2 N_2 O_{(g)} \xrightarrow{Pt} 2 N_{2(g)} + O_{2(g)}$
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What is the half-life of a first-order reaction if the rate constant is $4.2 \times 10^{-2} \text{ day}^{-1}$ (in $\text{ days}$)?
$A$ first order reaction is found to have a rate constant,$k = 5.5 \times 10^{-14} \ s^{-1}$. The half life of reaction is . . . . . . .
In a first-order reaction,the concentration of reactant $X$ decreases from $0.1 \, M$ to $0.005 \, M$ in $40 \, min$. What will be the rate of reaction when the concentration of $X$ is $0.01 \, M$?
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View SolutionWhat is the numerical value of the rate constant of a first-order reaction that is $20 \%$ completed in $10 \ min$ (in $min^{-1}$)?
For the first order reaction $A \rightarrow 2B$,$1 \ mole$ of reactant $A$ gives $0.2 \ moles$ of $B$ after $100 \ minutes$. The half-life of the reaction is $..... \ min$. [Use: $\ln 2 = 0.69, \ln 10 = 2.3$]
DifficultJEE MAIN 2021
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