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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 × 10“ mol/L. s. 2HI (g) →H2 (g) + I2 (g) Rate k = 1.22x104 mol/L. s. At i. a-If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. i. How long will it take for all of the 0.250 M HI to decompose?

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“ mol/L. s. 2HI (g) →H2 (g) + I2 (g) Rate k = 1.22x104 mol/L. s. At i. a-If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. i. How long will it take for all of the 0.250 M HI to decompose?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 × 10“ mol/L. s. 2HI (g) →H2 (g) + I2 (g) Rate k = 1.22x104 mol/L. s. At i. a-If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. i. How long will it take for all of the 0.250 M HI to decompose?
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 × 10“ mol/L. s. 2HI (g) →H2 (g) + I2 (g) Rate k = 1.22x104 mol/L. s. At i. a-If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. i. How long will it take for all of the 0.250 M HI to decompose?
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