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 × 10¬4 mol/L·s. Au 2 HI(9) Н2 (9) + 12(9) A[HI] = k = 1.20 × 10¬ª mol/L · s At Rate = - a. If the initial HI concentration was 0.500 mol/L, calculate the concentration of HI at 23 minutes after the start of the reaction. Concentration = M b. How long will it take for all of the 0.500 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 × 10¬4 mol/L·s. Au 2 HI(9) Н2 (9) + 12(9) A[HI] = k = 1.20 × 10¬ª mol/L · s At Rate = - a. If the initial HI concentration was 0.500 mol/L, calculate the concentration of HI at 23 minutes after the start of the reaction. Concentration = M b. How long will it take for all of the 0.500 M HI to decompose? Time = min
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 24PS: Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is...
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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 (g) + I2 (g)
A[HI]
Rate
k =
= 1.20 × 10- mol/L · s
At
a. If the initial
HI concentration was 0.500 mol/L, calculate the concentration of
HI at 23 minutes after the start of the reaction.
Concentration =
M
b. How long will it take for all of the 0.500 M
HI to decompose?
Time =
min](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fed7d8611-f555-47eb-8eb5-98565b9bae06%2F06f0bd61-cace-4e6f-b1d1-bf102198c456%2F1wmts9_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 (g) + I2 (g)
A[HI]
Rate
k =
= 1.20 × 10- mol/L · s
At
a. If the initial
HI concentration was 0.500 mol/L, calculate the concentration of
HI at 23 minutes after the start of the reaction.
Concentration =
M
b. How long will it take for all of the 0.500 M
HI to decompose?
Time =
min
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