For the gaseous reaction 3H₂ + N₂ ⇌ 2NH₃ given are the following no. of moles at equilibrium nH₂ = 0.24 mol, nN₂=0.08 mol, and nNH₃=0.84 mol starting with 1 mole of ammonia. The total pressure created by the system is 2.5 atm at a temperature of 38 °C. Find: a.) total # of moles in equilibrium and partial pressure b.) equilibrium constant of the system c.) standard free energy of the system assuming that gases behave ideally
For the gaseous reaction 3H₂ + N₂ ⇌ 2NH₃ given are the following no. of moles at equilibrium nH₂ = 0.24 mol, nN₂=0.08 mol, and nNH₃=0.84 mol starting with 1 mole of ammonia. The total pressure created by the system is 2.5 atm at a temperature of 38 °C. Find: a.) total # of moles in equilibrium and partial pressure b.) equilibrium constant of the system c.) standard free energy of the system assuming that gases behave ideally
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
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 10ALQ: In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What...
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For the gaseous reaction 3H₂ + N₂ ⇌ 2NH₃ given are the following no. of moles at equilibrium nH₂ = 0.24 mol, nN₂=0.08 mol, and nNH₃=0.84 mol starting with 1 mole of ammonia. The total pressure created by the system is 2.5 atm at a temperature of 38 °C. Find:
a.) total # of moles in equilibrium and partial pressure
b.) equilibrium constant of the system
c.) standard free energy of the system assuming that gases behave ideally
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