JEE Main & Advanced JEE Main Solved Paper-2016

  • question_answer
    Decomposition of \[{{H}_{2}}{{O}_{2}}\]follows a first order reaction. In fifty minutes the concentration of \[{{H}_{2}}{{O}_{2}}\]decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of \[{{H}_{2}}{{O}_{2}}\]reaches 0.05 M, the rate of formation of \[{{O}_{2}}\]will be :- [JEE Main Solved Paper-2016 ]

    A) \[\text{1}.\text{34}\times \text{1}{{0}^{\text{2}}}\text{mol mi}{{\text{n}}^{\text{1}}}\]

    B) \[\text{6}.\text{93}\times \text{1}{{0}^{\text{2}}}\text{mol mi}{{\text{n}}^{\text{1}}}\]

    C) \[\text{6}.\text{93}\times \text{1}{{0}^{\text{4}}}\text{mol mi}{{\text{n}}^{\text{1}}}\]

    D) \[\text{2}.\text{66 Lmi}{{\text{n}}^{\text{1}}}\text{at STP}\]

    Correct Answer: C

    Solution :

                    \[{{H}_{2}}{{O}_{2(aq)}}\xrightarrow[{}]{{}}{{H}_{2}}{{O}_{(aq)}}+\frac{1}{2}{{O}_{2}}(g)\] \[k=\frac{1}{t}\ln \left( \frac{{{a}_{0}}}{{{a}_{t}}} \right)\]                            \[=\frac{1}{50}\ln \left( \frac{0.5}{0.125} \right)\] \[=\frac{1}{50}\ell \ln 4{{\min }^{-1}}\] \[\frac{\text{Rate of disappearance of }{{\text{H}}_{\text{2}}}{{O}_{2}}}{1}\] \[=\frac{\text{Rate of appearance of }{{O}_{2}}}{\frac{1}{2}}\] \[(Rate){{O}_{2}}=\frac{1}{2}\times (Rate){{H}_{2}}{{O}_{2}}\] \[=\frac{1}{2}k[{{H}_{2}}{{O}_{2}}]\]                       \[=\frac{1}{2}\times \frac{1}{50}\times \ell n4\times 0.05\] \[=\text{6}.\text{93}\times \text{1}{{0}^{\text{4}}}\text{M mi}{{\text{n}}^{\text{1}}}\]


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