The following reaction was monitored as a function of time: AB--->A +B
A plot of 1/[AB] versus time yields a straight line with slope 5.2 x 10^-2 M*s.
What is the value of the rate constant (k) for this reaction at this temperature?
Slope they give is = to rate constant (k)
5.2x10^-2
To find the rate constant (k) of the reaction, we need to use the rate equation and the given information.
The rate equation for the reaction AB → A + B is given by:
rate = k[AB]
Here, [AB] represents the concentration of AB at a given time, and k is the rate constant.
We are given that a plot of 1/[AB] versus time yields a straight line with a slope of 5.2 × 10^-2 M*s.
The rate is given by:
rate = - d[AB]/dt
Since 1/[AB] is linear with time, we can write it as:
1/[AB] = kt + C
Where k is the rate constant and C is a constant of integration.
Since the slope of the line is given as 5.2 × 10^-2 M*s, we can equate it to the rate constant (k):
5.2 × 10^-2 M*s = k
Therefore, the value of the rate constant (k) for this reaction at this temperature is 5.2 × 10^-2 M*s.