In: Chemistry
How do you find the rate constant here?
trials | [I] | [H2O2] | [H] | temp (C) | Rate (M/s) |
1 | 8.53*10^-3 | 1.03*10^-1 | 0.333 | 21.5 | 5.33*10^-4 |
2 | 8.53*10^-3 | 1.03*10^-1 | 0.333 | 15 | 4.3*10^-4 |
3 | 8.53*10^-3 | 1.03*10^-1 | 0.333 | 42 | 2.17*10^-3 |
In chemical kinetics a reaction rate constant,
k or
, quantifies the rate of a chemical reaction.[1]
For a reaction between reactants A and B to form product C
the reaction rate is often found to have the form:
Here k(T) is the reaction rate constant that depends on temperature. [A] and [B] are the concentrations of substance A in moles per volume of solution assuming the reaction is taking place throughout the volume of the solution. (For a reaction taking place at a boundary one would use instead moles of A or B per unit area).
trials | [I] | [H2O2] | [H] | temp (C) | Rate (M/s) |
1 | 8.53*10^-3 | 1.03*10^-1 | 0.333 | 21.5 | 5.33*10^-4 |
2 | 8.53*10^-3 | 1.03*10^-1 | 0.333 | 15 | 4.3*10^-4 |
3 | 8.53*10^-3 | 1.03*10^-1 | 0.333 | 42 | 2.17*10^-3 |
1.
T is
in K
on solving we get k= 6.827*10-3 L2M-1s-1
2.
on puttin values and solving
k = 6.981*10-3 L2M-1s-1
3.
on puttin values and solving
k = 6.383*10-3 L2M-1s-1