🤓 Based on our data, we think this question is relevant for Professor Nash's class at PURDUE.
Consider the gas-phase reaction: H2(g) + I2(g) → 2 HI(g)
The reaction was experimentally determined to be first order in H2 and first order in I2. Consider the proposed mechanisms.
Proposed mechanism I: H2(g) + I2(g) → 2 HI(g) Single step
Proposed mechanism II:
I2(g) → 2 I(g) Fast
H2(g) + 2 I(g) → 2 HI(g) Slow
Show that the first of the proposed mechanisms is valid.
Rate Law represents an equation for a chemical reaction that connects the reaction rate with the concentrations or pressures of the reactants and the rate constant.
Rate Law = k[A]x[B]y
Where k is the rate constant
A and B are reactants
x and y are reactant orders
The proposed mechanism 1 is:
H2(g) + I2(g) → 2 HI(g) (single step)