15. Chemical Kinetics
Rate Law
Multiple Choice
Multiple ChoiceThe concentration of N2O was monitored at a constant temperature as a function of time for the reaction below.
N2O (g) → N2 (g) + ½ O2 (g)
Time (s) | Molar Concentration [N2O] |
---|---|
0 | 0.500 M |
20 | 0.382 M |
40 | 0.310 M |
60 | 0.260 M |
80 | 0.224 M |
A
rate = k[N2O]
B
rate = k[N2O][N2][O2]½
C
rate = k[ N2O]0
D
rate = k[ N2O]2
E
rate = k[N2][O2]½
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