Chemical Kinetics and Nuclear ChemistryEasy
Question
For The Reaction,
N2O5(g) → 2NO2(g) + 1/2 O2(g)
the value of rate of disappearance of N2O5 is given as 6.25 × 10-3 mol L-1 s-1. The rate of formation of NO2 and O2 is given respectively as -
N2O5(g) → 2NO2(g) + 1/2 O2(g)
the value of rate of disappearance of N2O5 is given as 6.25 × 10-3 mol L-1 s-1. The rate of formation of NO2 and O2 is given respectively as -
Options
A.6.25 × 10-3 mol L-1 s-1 and 6.25 × 10-3 mol L-1 s-1
B.1.25 × 10-2 mol L-1 s-1 and 3.125 × 10-3 mol L-1 s-1
C.6.25 × 10-3 mol L-1 s-1 and 3.125 × 10-3 mol L-1 s-1
D.1.25 × 10-2 mol L-1 s-1 and 3.125 × 10-3 mol L-1 s-1
Solution
Rate of disappearance of reactant = rate of appearance of products
or
=
For the reaction,
N2O5(g) → 2NO2(g) + 1/2O2
∴
= 2 × 6.25 × 10-3 mol L-1 s-1
= 12.5 × 10-3 mol L-1 s-1
= 1.25 × 10--2 mol L-1 s-1
= 3.125 × 10-3 mol L-1 s-1
or
=
For the reaction,
N2O5(g) → 2NO2(g) + 1/2O2
∴
= 2 × 6.25 × 10-3 mol L-1 s-1
= 12.5 × 10-3 mol L-1 s-1
= 1.25 × 10--2 mol L-1 s-1
= 3.125 × 10-3 mol L-1 s-1
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