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CBSE Class 12 Chemistry 2023 Delhi Set 1 Solved Paper

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Question : 26
Total: 35
SECTION - C
(a) For the reaction
2N2O5(g)→4NO2(g)+O2(g) at 318K
Calculate the rate of reaction if rate of disappearance of N2O5(g) is 1.4×10−3ms−1.
(b) For a first order reaction derive the relationshipt99%=2t90%
Solution:     👈: Video Solution
(a) 2~N2O5→4NO2+O2
−
1
2
d[N2O5]
dt
=+
1
4
d[NO2]
dt
=+
d[O2]
dt
=2×
1
4
×1.4×10−3 [Rate of disappearance =1.4×10−3ms−1]
=0.7×10−3ms−1
(b) For a first order of reaction
t=
2.303
K
‌log‌
a
a−x
t99%=
2.303
K
‌log‌
100
1
=
2.303
K
‌log‌100
=
2.303×2
K
=
4.606
K
and t90%=
2.303
K
‌log‌
a
a−x
=
2.303
K
‌log‌10=
2.303
K
t99%
t90%
=2
t99%=2t90%.
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