InterviewSolution
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InterviewSolution
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For the reaction `N_(2)O_(5) rarr 2NO_(2) + (1)/(2) O_(2)`, the rate of disappearance of `N_(2)O_(5)` is `6.25 xx 10^(-3) "mol L"^(-1) s^(-1)`. The rate of formation of `NO_(2)` and `O_(2)` will be respectively.A. `6.25xx10^(-3)molL^(-1)S^(-1)and 6.25xx10^(-3)molL^(-1)S^(-1)`B. `1.25xx10^(-2)molL^(-1)S^(-1)and 3.125xx10^(-3)molL^(-1)S^(-1)`C. `6.25xx10^(-3)molL^(-1)S^(-1)and 3.125xx10^(-3)molL^(-1)S^(-1)`D. `1.25xx10^(-2)molL^(-1)S^(-1)and 6.25xx10^(-3)molL^(-1)S^(-1)` |
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Answer» Correct Answer - B key idea rate of disappearance of reactant = rate of appearance of product `or (1)/(" Stoichiometric coefficient of reactant")(d"[ reactant]")/(dt)` `=+(1)/(" Stoichiometric coefficient of reactant")(d"[product]")/(dt)` for the reaction , `N_(2) O_(5)(g) to 2NO_(3) (g) +(1)/(2)O_(2)(g)` ` (-d[N_(2)O_(5)])/(dt)=+(1)/(2)(d[NO_(2)])(dt)=+(2d[O_(2)])/(dt)` `therefore (d[NO_(2)])/(dt) =-2(d[N_(2)O_(5)])/(dt)` `=2xx6.25xx10^(-3)molL^(-1)S^(-1)` `=12.5xx10^(-3)mol L^(-1)S^(-1)` `= 1.25xx10^(-2)mol L^(-1)S^(-1)` `(d[O_(2)])/(dt) =- (d[N_(2)O_(5)])/(dt ) xx(1)/(2 ) ` `=(6.25xx10^(-3)mol L^(-1)S^(-1))/(2) ` ` =3.125xx10^(-3)molL^(-1) S^(-1)` |
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