Decomposition of phosphine $(PH_3)$ at $120^{\circ}C$ proceeds according to the equation: $4PH_3(g) \to P_4(g) + 6H_2(g)$ It is found that this reaction follows the following rate equation: Rate $= k[PH_3]$ The half-life of $PH_3$ is $37.9\;s$ at $120^{\circ}C.$ (i) How much time will be required for $\large\frac{3}{4}$ of $PH_3$ to decompose? (ii) What fraction of the original amount of $PH_3$ will remain undecomposed after 1 minute?

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