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Ammonium iodide, a solid, decomposes to give NH3(g) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(g) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH₂I(s) NH3(g) + HI(g) K= PHI atm

Ammonium iodide, a solid, decomposes to give NH3(g) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(g) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH₂I(s) NH3(g) + HI(g) K= PHI atm

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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Ammonium iodide, a solid, decomposes to give NH3(9) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(9) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH4I(s) NH3(g) + HI(g) PHI = atm
Transcribed Image Text:Ammonium iodide, a solid, decomposes to give NH3(9) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(9) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH4I(s) NH3(g) + HI(g) PHI = atm
The reaction 2SO3(g)2SO₂(g) + O2(g) has an equilibrium constant Kp (in terms of pressures) at 877 °C of 2.74. Calculate the concentration of SO₂ that will be present at 877 °C in equilibrium with SO3 (at a concentration of 8.56x 10-3 mol L-¹) and O₂ (at a concentration of 8.10x10-3 mol L-1 Submit Answer 5 question attempts remaining [SO₂] =
Transcribed Image Text:The reaction 2SO3(g)2SO₂(g) + O2(g) has an equilibrium constant Kp (in terms of pressures) at 877 °C of 2.74. Calculate the concentration of SO₂ that will be present at 877 °C in equilibrium with SO3 (at a concentration of 8.56x 10-3 mol L-¹) and O₂ (at a concentration of 8.10x10-3 mol L-1 Submit Answer 5 question attempts remaining [SO₂] =
Expert Solution
Step 1

Given:

For equation:
NH4I(s)→ NH3(g) + HI(g) 

Total pressure  = 1.07 atm Partial pressure of NH3= 1.37 atm

 

 

 

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