Which of the following is an example of a first-order reaction?
- A$CH_3CHO_{(g)} \rightarrow CH_{4_{(g)}} + CO_{(g)}$
- B$2NO_{2_{(g)}} + F_{2_{(g)}} \rightarrow 2NO_2F_{(g)}$
- C$2NO_{(g)} + 2H_{2_{(g)}} \rightarrow N_{2_{(g)}} + 2H_2O_{(g)}$
- D$2H_2O_{2_{(aq)}} \rightarrow 2H_2O_{(l)} + O_{2_{(g)}}$
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Identify True $(T)$ and False $(F)$ statements of the following for a first order reaction $R \rightarrow P$.
$(i) \ t_{1/2} \propto [R]_0^0$
$(ii) \ t_{1/2} = \frac{0.693}{k}$
$(i) \ t_{1/2} \propto [R]_0^0$
$(ii) \ t_{1/2} = \frac{0.693}{k}$
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View SolutionFor the reaction $A \rightarrow B$,the following graph was obtained. The time required (in seconds) for the concentration of $A$ to reduce to $2.5 \ g \ L^{-1}$ (if the initial concentration of $A$ was $50 \ g \ L^{-1}$) is $........$ (Nearest integer). Given: $\log 2 = 0.3010$.
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View SolutionSucrose hydrolyses in acidic medium into glucose and fructose by first order rate law with $t_{1/2} = 3 \text{ hours}$. The percentage of sucrose remaining after $6 \text{ hours}$ is . . . . . . . (Nearest integer) (Given: $\log 2 = 0.3010$ and $\log 3 = 0.4771$)
Radioactive decay is a
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View SolutionWhat is the half-life of a first-order reaction if the time required to decrease the concentration of the reactant from $0.8 \text{ M}$ to $0.2 \text{ M}$ is $12 \text{ hours}$ (in $\text{ hours}$)?
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