We’re being asked to determine the overall rate-law expression for the reaction below:
2 NO2Cl(g) → 2 NO2(g) + Cl2(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
When a reaction mechanism is given, the rate law can be determined using the slow step in the reaction mechanism.
Consider the following mechanism for the overall reaction 2NO2Cl(g) → 2NO2(g) + Cl2(g).
Step1 NO2Cl NO2 + Cl fast
Step2 NO2Cl + Cl NO2 + Cl2 slow
If this mechanism were correct, what would be the overall rate-law expression?
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What scientific concept do you need to know in order to solve this problem?
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Based on our data, we think this problem is relevant for Professor TBA's class at UW-SEATTLE.