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Question
For a reaction 2N2O5(g)→4NO2(g)+O2(g) , the rate and rate constant are 1.02×10−4 mol L−1 s−1 and 3.4×10−5 s−1 respectively. The concentration of N2O5 at this time will be:
For a reaction 2N2O5(g)→4NO2(g)+O2(g) , the rate and rate constant are 1.02×10−4 mol L−1 s−1 and 3.4×10−5 s−1 respectively. The concentration of N2O5 at this time will be:
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Solution
The correct option is B 3 mol/L
The given reaction is
2N2O5→4NO2+O2
Given, rate=R=1.02×10−4 mol L−1s−1
Rate constant = k=3.010 s−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
The given reaction is
2N2O5→4NO2+O2
Given, rate=R=1.02×10−4 mol L−1s−1
Rate constant = k=3.010 s−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
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