Use the Kelerences to access importast valees if needed for this question The fo

Question

Use the Kelerences to access importast valees if needed for this question The following initial rate data are for the reaction of ICI with hydrogen ICI+H+2 HCI Experiment ICl, M Instial Rate, M s 5.79 103 1.16 102 2.31 10 2 62 102 59 10-2 0.172 192 192 383 50 10-2 172 Complete the rate law for this reaction in the box below Use the form kJA)"B)", where "1' is understood for m or n and concentrations taken to the zero power do not appear Don't enter I for m or n From these data, the rate constant is'

Explanation / Answer

2 ICI     +     H2     ------>     I2     + 2 HCl

Rate = k [ICI]m [H2]n

Now,

Considering experiment (1) and (2), Keeping [H2] concentration constant and increasing the concentration of [ICI] by two times the rate increases by two times.

2 x Rate = k [2 ICI]m [H2]n

Or, 2 x Rate = k 2m [ICI]m [H2]n

Or, 2 x Rate = 2m (k [ICI]m [H2]n )

Or, 2 = 2m

Or, m = 1

Again, considering experiment (1) and (3), Keeping [ICI] concentration constant and increasing the concentration of [H2] by four times the rate increases by two times.

4 x Rate = k [ICI]m [2H2]n

Or, 4 x Rate = k 2n [ICI]m [H2]n

Or, 4 x Rate = 2n (k [ICI]m [H2]n )

Or, 4 = 2n

Or, n = 2

So, the overall rate equation is expressed as

Rate = k [ICI]1 [H2]2

Rate = k [ICI] [H2]2

Now, substituting the values from experiment 2 in the rate equation, we get;

1.16 x 10-2 Ms-1= k (0.172 M) x (0.192 M)2

Or, 1.16 x 10-2 Ms-1 = k (0.172 M) x (0.192 M)2

Or, 1.16 x 10-2 Ms-1 = k (6.34 x 10-3) M3

k = [1.16 x 10-2 Ms-1] / [(6.34 x 10-3) M3]

k = 1.83 M-2s-1

Related Questions

Navigate

• Browse (All)
• Browse U
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.