the decomposition of h2o2 is first order reation following up the decom position it was found that the remaining h2o2 after 45 min was 15 units from the original concentration57.5 unit calculate the rate constant
To calculate the rate constant for the first-order decomposition reaction of H2O2, we can use the formula for a first-order reaction:
ln([A]t/[A]0) = -kt
Where:
[A]t = concentration of H2O2 at time t
[A]0 = initial concentration of H2O2
k = rate constant
t = time
From the given information:
[A]t = 15 units
[A]0 = 57.5 units
t = 45 min
Plugging in the values, the equation becomes:
ln(15/57.5) = -k * 45
We can rearrange the equation to solve for the rate constant (k):
-k * 45 = ln(15/57.5)
Divide both sides by -45:
k = -ln(15/57.5) / 45
Now let's calculate the rate constant using this formula:
k = -ln(15/57.5) / 45
Using a scientific calculator or software, evaluate the natural logarithm (ln) of (15/57.5). Then, divide the result by 45. You should obtain the value for the rate constant (k) of the reaction.