At $$300 \mathrm{~K}$$, the half-life period of a gaseous reaction at an initial pressure of $$40 \mathrm{~kPa}$$ is 350 s. When pressure is $$20 \mathrm{~kPa}$$, the half-life period is 175 s. What is the order of the reaction?
For a reaction, $$2 A+B \longrightarrow$$ products, If concentration of $$B$$ is kept constant and concentration of $$A$$ is doubled then rate of reaction is
A first order reaction proceeds to $$90 \%$$ completion. What will be the approximate time taken for $$90 \%$$ completion in relation to $$t_{1 / 2}$$ of the reaction?
For a reaction of the type, $$2 \mathrm{X}+\mathrm{Y} \rightarrow \mathrm{A}+\mathrm{B}$$, the following is the data collected:
| Experiment | $$\mathrm{[X]}$$ | $$\mathrm{[Y]}$$ | Initial rate of formation of A |
|---|---|---|---|
| 1 | 0.2 | 0.2 | $$12.0\times10^{-3}$$ |
| 2 | 0.6 | 0.4 | $$\mathrm{14.4\times10^{-2}}$$ |
| 3 | 0.6 | 0.8 | $$5.76\times10^{-1}$$ |
| 4. | 0.8 | 0.2 | $$\mathrm{4.8\times10^{-2}}$$ |
What is the overall order of the reaction?
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