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The decomposition of N_(2)O_(5) in carbon tetrachloride solution was studied N_(2)O_(5)("solution")to2NO_(2)("solution")+(1)/(2)O_(2)(g) The reaction has been found to be first order and the rate constant is found to be 6.2xx10^(-4)s^(-1). Calculate the rate of reaction when (a)[N_(2)O_(5)]=1.25" mol L"^(-1)" and "(b)[N_(2)O_(5)]=0.25" mol L"^(-1). (c) What concentration of N_(2)O_(5) would give a rate of 2.4xx10^(-3)" mol L"^(-1)s^(-1)? |
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Answer» Solution :(a) Rate `=k[N_(2)O_(5)]=(6.2xx10^(-4)s^(-1))(1.25" mol L"^(-1))=7.75xx10^(-4)" mol L"^(-1)s^(-1)` (B) Rate `=(6.2xx10^(-4)s^(-1))(0.25" mol L"^(-1))=1.55xx10^(-4)" mol L"^(-1)s^(-1)` (c) `2.4xx10^(-3)" mol L"^(-1)s^(-1)=(6.2xx10^(-4)s^(-1))[N_(2)O_(5)]" or "[N_(2)O_(5)]=3.87" mol L"^(-1).` |
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