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Question
For the reaction, N2O5(g)→NO2(g)+12O2(g) The value of rate of disappearance of N2O5 is given as 6.25×10−3molL−1s−1. The rate of formation of NO2 and O2 is given respectively as:
For the reaction, N2O5(g)→NO2(g)+12O2(g) The value of rate of disappearance of N2O5 is given as 6.25×10−3molL−1s−1. The rate of formation of NO2 and O2 is given respectively as:
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Solution
The correct option is B 1.25×10−2molL−1s−1and3.125×10−3molL−1s−1
Rate of disappearance of reactant = rate of appearance of product
Or -1Stoichiometric coefficient of reactantd[reactant]dt
+1Stoichiometric coefficient of productd[product]dt
For the reaction,
N2O5(g)→2NO2(g)+12O2(g)−d[N2O5]dt=+12d[NO2]dt=+2d[O2]dt
∴d[NO2]dt=−2d[N2O5]dt=2×6.25×10−3molL−1s−1=12.5×10(−3)molL−1s−1
=1.25×10−2molL−1s−1d[O2]dt=−d[N2O5]dt×12=6.25×10−3molL−1s−12=3.125×10−3molL−1s−1
1.25×10−2molL−1s−1and3.125×10−3molL−1s−1
Rate of disappearance of reactant = rate of appearance of product
Or -1Stoichiometric coefficient of reactantd[reactant]dt
+1Stoichiometric coefficient of productd[product]dt
For the reaction,
N2O5(g)→2NO2(g)+12O2(g)−d[N2O5]dt=+12d[NO2]dt=+2d[O2]dt
∴d[NO2]dt=−2d[N2O5]dt=2×6.25×10−3molL−1s−1=12.5×10(−3)molL−1s−1
=1.25×10−2molL−1s−1d[O2]dt=−d[N2O5]dt×12=6.25×10−3molL−1s−12=3.125×10−3molL−1s−1
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