The following reaction is monitored against time; AB ⇒ A + B The plot of time against 1 / [AB] gives a line with a slope of -0.0045 / s. a) The value of the rate constant of the reaction, b) Kinetic expression for reaction (rate law), c) The half-life of the reaction since the initial concentration is 0.55 M, d) the concentrations of A and B after 75 s when the initial concentration of AB is 0.250 M and there is no product initially, which option is given correctly? A)Rate constant: 0.0045 Speed law: R = k [AB] 2 Half life: 404 s [A]: 0.020 [B]: 0.020 B)Rate constant: -0.0045 Speed law:
The following reaction is monitored against time; AB ⇒ A + B The plot of time against 1 / [AB] gives a line with a slope of -0.0045 / s. a) The value of the rate constant of the reaction, b) Kinetic expression for reaction (rate law), c) The half-life of the reaction since the initial concentration is 0.55 M, d) the concentrations of A and B after 75 s when the initial concentration of AB is 0.250 M and there is no product initially, which option is given correctly?
A)Rate constant: 0.0045 Speed law: R = k [AB] 2 Half life: 404 s [A]: 0.020 [B]: 0.020
B)Rate constant: -0.0045 Speed law: R = k [AB] Half life: 200 s [A]: 0.230 [B]: 0.230
C)Rate constant: -0.0045 Speed law: R = k [AB] 2 Half life: 300 s [A]: 0.250 [B]: 0.250
D)Rate constant: -0.0045 Speed law: R = k [A] [B] Half life: 300 s [A]: 0.230 [B]: 0.230
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