For a reaction 2N2O5(g)→4NO2(g)+O2(g) , the rate and rate constant are 1.02×10−4molL−1s−1 and 3.4×10−5s−1 respectively. The concentration of N2O5 at this time will be:
A
1.732 mol/L
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B
3 mol/L
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C
1.02×10−4 mol/L
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D
3.2×105 mol/L
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Solution
The correct option is B 3 mol/L The given reaction is 2N2O5→4NO2+O2
Given, rate=R=1.02×10−4molL−1s−1
Rate constant = k=3.010s−1
Reaction follows 1storder kinetics as unit of k is s−1
Rate = k[N2O5] 1.02×10−4 = (3.4×10−5)[N2O5] [N2O5]=3 mol/L