Calculate the rate constant, k, for the reaction 2H2O2(l) --> 2H2O(l) + O2(g)
Using the rate, - 0.02 mol/L.min H2O2, and the initial concentration, [H2O2] = 0.5 mol/L
Question 7 options:
- 25/min
25/min
- 0.04/min
0.04/min
To calculate the rate constant, k, we can use the rate equation for a first-order reaction:
rate = k * [H2O2]
Given:
Rate = -0.02 mol/L.min (negative sign indicates the decrease in concentration over time)
[H2O2] = 0.5 mol/L
Substituting the given values into the rate equation:
-0.02 mol/L.min = k * 0.5 mol/L
Solving for k:
k = (-0.02 mol/L.min) / (0.5 mol/L)
k = -0.04 min^-1
Therefore, the rate constant, k, for the reaction is -0.04/min.
To calculate the rate constant, k, for the given reaction, we can use the rate equation:
Rate = k[H2O2]^m
Here, the rate is given as -0.02 mol/L.min (negative sign indicates the reactant is being consumed), the initial concentration of H2O2 ([H2O2]) is 0.5 mol/L, and the stoichiometric coefficient of H2O2 in the balanced equation is 2.
To solve for the rate constant, we can rearrange the rate equation:
Rate = k[H2O2]^2
Plugging in the given values:
-0.02 mol/L.min = k * (0.5 mol/L)^2
Simplifying:
-0.02 mol/L.min = k * 0.25 mol^2/L^2
Now, we can isolate the rate constant, k:
k = (-0.02 mol/L.min) / (0.25 mol^2/L^2)
k = -0.08 L/mol.min
It is important to note that the rate constant should always have a positive value. Taking the absolute value, the rate constant is 0.08 L/mol.min.
So, the closest option to the calculated rate constant is 0.08/min, which is not one of the provided options. Therefore, none of the options given is the correct answer.
I believe this is a first order with respect to H2O2.
rate = k(H2O2)^1