Question

The reaction H₂(g) + I₂(g) → 2 HI (g) is first order in both hydrogen and iodine. It is therefore referred to as second order overall. Its rate constant for the formation of HI (g) at 400 ◦C is 2.34 × 10−2 · lit · mol−1 · sec−1 and its activation energy is 150 KJ/mol.

Use the rate law to estimate how long it takes to form 0.1 mole of HI(g) if I start by putting 2 moles of H₂ and 2 moles of I₂ in a 10 liter box and allow them to react. Note that if we were considering this rigorously we would need to compute Keq and satisfy ourselves that the reaction actually does proceed at least as far as making 0.1 mole of HI(g). For the purposes of this problem, you can assume that the reaction goes to completion eventually.

Answer 1

2 Given Reaction Rate-of-to df oc Inmal No of moles of H, tg) = 2m- = 2mle 2 male of No. males-of-긔ig)--emale O-2 M Initia。。-2M finul (0.2-x)M (0-2-x) M dre

males of HI No o. I mole mmed-=- っc = o.oos M