The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to HI. The rate defined below is constant at 1.20 x 10-4 mol/L-s. Au 2 HI(g) H2 (9) + I (g) A[H] = k = 1.20 x 104 mol/L ·s At Rate = a. If the initial HI concentration was 0.650 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. Concentration = M b. How long will it take for all of the 0.650 M HI to decompose? Time = min
The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to HI. The rate defined below is constant at 1.20 x 10-4 mol/L-s. Au 2 HI(g) H2 (9) + I (g) A[H] = k = 1.20 x 104 mol/L ·s At Rate = a. If the initial HI concentration was 0.650 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. Concentration = M b. How long will it take for all of the 0.650 M HI to decompose? Time = min
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 50E: The decomposition of hydrogen iodide on finely divided gold at 150C is zero order with respect to...
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![The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to
HI. The rate defined below is constant at 1.20 x 10-4 mol/L-s.
Au
2 HI(g) H2 (9) + I (g)
A[H]
= k = 1.20 x 104 mol/L ·s
At
Rate =
a. If the initial HI concentration was 0.650 mol/L, calculate the concentration of HI at 25 minutes
after the start of the reaction.
Concentration =
M
b. How long will it take for all of the 0.650 M HI to decompose?
Time =
min](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa0bb861a-a74a-4663-bbeb-0fca4422e7c0%2Fde4e3f52-06b0-4c7a-9f3b-ede55679fac2%2Fde0meu1j_processed.png&w=3840&q=75)
Transcribed Image Text:The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to
HI. The rate defined below is constant at 1.20 x 10-4 mol/L-s.
Au
2 HI(g) H2 (9) + I (g)
A[H]
= k = 1.20 x 104 mol/L ·s
At
Rate =
a. If the initial HI concentration was 0.650 mol/L, calculate the concentration of HI at 25 minutes
after the start of the reaction.
Concentration =
M
b. How long will it take for all of the 0.650 M HI to decompose?
Time =
min
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