Mention True $(T)$ and False $(F)$ statements for the following equations related to the reaction $R \to P$:
$I. [R] = -kt + [R]_0$
$II. [R] = kt + [R]_0$
$I. [R] = -kt + [R]_0$
$II. [R] = kt + [R]_0$
- A$I-T, II-F$
- B$I-F, II-T$
- C$I-T, II-T$
- D$I-F, II-F$
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Which of the following is correct with respect to the graph given?
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$
$[R] = \text{Concentration at time } 't'$
$[R]_0 = \text{Initial concentration}$
Mention True $(T)$ and False $(F)$ statement of the following for reaction $R \to P$.
Rate $= -\frac{d[R]}{dt} = k[R]^0$
Rate $= -\frac{d[R]}{dt} = k$
Rate $= -\frac{d[R]}{dt} = k[R]^0$
Rate $= -\frac{d[R]}{dt} = k$
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View SolutionThe unit of velocity constant in case of zero order reaction is
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View SolutionFor the zero order reaction $2A \rightarrow B + 3C$,if the rate constant $K = 3.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,what will be the rate of production of $C$?
Which of the following plots is correct for a zero-order reaction?
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