We’re being asked to calculate the rate law and the value of the rate constant (k) based on the reaction and data given.
Given reaction: CH3Cl(g) + 3 Cl2(g) → CCl4(g) + 3 HCl(g)
Recall that the rate law only focuses on the reactant concentrations and has a general form of:
k = rate constant
A & B = reactants
x & y = reactant orders
We’re going to calculate the rate law and the rate constant using the following steps:
The data below were collected for the following reaction:
CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g)
CH3Cl(M) Cl 2(M) Initial Rate(M/s)
0.050 0.050 0.014
0.100 0.050 0.029
0.100 0.100 0.041
0.200 0.200 0.115
Calculate the value of the rate constant, k.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Rate Law concept. You can view video lessons to learn Rate Law. Or if you need more Rate Law practice, you can also practice Rate Law practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Stolley's class at UTAH.