The reaction Cl + CH
4 HCl + CH
3 has been studied by forming Cl atoms with a laser pulse in excess methane, and observing the concentration of HCl as a function of time.
(a) Show that the HCl concentration, [itex]c_{HCl}[/itex], varies with time t as
[tex]c_{HCl} = c_{HCl,t=\infty} \cdot (1 - e^{-k_1 \cdot c_{CH_4} \cdot t})[/tex]
where [itex]c_{CH_4}[/itex] is the methane concentration, [itex]c_{HCl,t=\infty}[/itex] is the concentration of HCl at t=∞ and [itex]k_1[/itex] is the rate constant.
(b) The following data apply to the reaction at 298 K with [CH
4] = 10
15 molecule cm
-3.
t / ms, [HCl] / 10
10 molecule cm
-32, 0.57
4, 1.05
8, 1.74
12, 2.19
16, 2.46
∞, 3.00
Evaluate k1.
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I don't have a clue on the first part. Especially why there is no dependence on Cl's concentration.
On the second, I can obviously rearrange for k
1 and plug in the values for a certain set, but we've been given 5 sets of data in addition to the t=∞ result, which to me suggests that we should use more than one. I get either 1.08·10
-16 molecule
-1·cm
3·s
-1 or 1.07·10
-16 molecule
-1·cm
3·s
-1 depending on which set I use, but a more advanced method is unclear to me.