A) \[6.35\times {{10}^{-3}}\,\text{mol}\,{{L}^{-1}}{{s}^{-1}}\]
B) \[5.15\times {{10}^{-5}}\,\text{mol}\,{{\text{L}}^{-1}}{{s}^{-1}}\]
C) \[3.85\times {{10}^{-4}}\,\text{mol}\,{{\text{L}}^{-1}}\,{{s}^{-1}}\]
D) \[7.75\times {{10}^{-4}}\,\text{mol}\,{{\text{L}}^{-1}}{{s}^{-1}}\]
Correct Answer: D
Solution :
\[{{N}_{2}}O\]in \[CC{{l}_{4}}\]solution \[\to 2N{{O}_{2}}(soln.)+\frac{1}{2}{{O}_{2}}\] Rate of this reaction is given as Rate = Rate constant \[\times \,{{[{{N}_{2}}{{O}_{5}}]}^{1}}\] \[[{{N}_{2}}{{O}_{5}}]=\]Concentration of \[{{N}_{2}}{{O}_{5}}.\] On putting the values of\[[{{N}_{2}}{{O}_{5}}]\]and rate constant we get, Rate \[=6.2\times {{10}^{-4}}{{s}^{-1}}\times 1.25\,\text{mol}\,{{\text{L}}^{-1}}\] \[=7.75\times {{10}^{-4}}\,mol\,{{L}^{-1}}{{s}^{-1}}.\] Hence, the correct option is (d).
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