Hint: It is not necessary to graph these data. (1) The observed half life for th

Question

Hint: It is not necessary to graph these data.

(1)
The observed half life for this reaction when the starting concentration is 1.12×10-2 M is s and when the starting concentration is 5.60×10-3 M is s.

(2)
The average rate of disappearance of NH3 from t = 0 s to t = 442 s is M s-1.

(3)
The average rate of disappearance of NH3 from t = 442 s to t = 662 s is M s-1.

(4)
Based on these data, the rate constant for this _______zerofirstsecond order reaction is M s-1.

B-

Explanation / Answer

Q1.

The observed half life for this reaction when the starting concentration is 1.12×10-2 M is s and when the starting concentration is 5.60×10-3 M is s.

From the table,

when A = 1.12*10^-2 then, half value is 0.56*10^-2 M, this is at t = 442 seconds

For A = 5.6*10^-3 ; half value is 2.8*10^-3 this is dt = 662-442 = 220 seconds

Q2

The average rate of disappearance of NH3 from t = 0 s to t = 442 s is M s-1.
Avg = Cfinal - Cinitial / Tfinal - Tinitial

Avg = (5.6*10^-3 - 1.12*10^-2)/(442) = 0.000012669 M/s of disappearance

Q3.

The average rate of disappearance of NH3 from t = 442 s to t = 662 s is M s-1.

Avg = Cfinal - Cinitial / Tfinal - Tinitial

Avg = (2.8*10^-3 - 5.6*10^-3)/(662-442) = 0.000012727 M/s of disappearance

The rate is always the same, so this means it must be constant

Therefore

Zero order,

Rate = K

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