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Solution: 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 stepProposed mechanism II:I2(g) → 2 I(g)          FastH2(g) + 2 I(g) → {uildreloverlongrightarrow} atop {uildrel { k_3} over ;} 2 HI(g)          SlowShow that the first of the proposed mechanisms is valid.

Problem

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) → HI(g)          Slow

Show that the first of the proposed mechanisms is valid.

Solution

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)


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