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  • For a reaction, <img alt="\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g}) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{g}), \text { rate }=5 \cdot 5 \times 10^{-14}\left[\mathrm{C}_{2} \mathrm{H}_{4}\right]" src="https://

For a reaction, \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g}) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{g}), \text { rate }=5 \cdot 5 \times 10^{-14}\left[\mathrm{C}_{2} \mathrm{H}_{4}\right].

(a) Write the unit of rate constant.

(b) Calculate its half-life  \left ( t_\frac{1}{2} \right ).

 

 

 

 
 
 
 
 

Answers (1)

\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g}) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{g}), \text { rate }=5 \cdot 5 \times 10^{-14}\left[\mathrm{C}_{2} \mathrm{H}_{4}\right](a) Unit of rate constant =s^{-1}

(b) Half life \left ( t_\frac{1}{2} \right )=?

\begin{aligned} t_{1 / 2} &=\frac{0.693}{k} \\ &=\frac{0.693}{5.5 \times 10^{-14}}=1.26 \times 10^{13} \mathrm{s} \end{aligned}

Posted by

Sumit Saini

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