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In the reversible reaction
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a
2k1k2[NO2]2
b
2k1[NO2]2 − 2k2[N2O4]
c
2k1[NO2]2 −k2[N2O4]
d
(2k1−k2)[NO2]
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Correct option is B
For the reaction, 2 NO2⇌k2k1N2O4, Given ,The rate of disappearance of NO2 =?For forward reaction rate= −12dNO2dt=dN2O4dt =k1[NO2]2 For backward reactionRate=−dN2O4dt=12dNO2dt=k2[N2O4]. Rate of disappearance of NO2 = (Rate of disappearance of NO2− Rate of appearance of NO2 )=2k1[NO2]2−2k[N2O4].Similar Questions
Rate law for from following data:
| S.No. | [A](M) | [B](M) | Rate(M./s) |
| 1. | 0.01 | 0.01 | 2.5 |
| 2. | 0.01 | 0.02 | 5 |
| 3. | 0.03 | 0.02 | 45 |
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