3. a. Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia. At 200 °C in a closed container, 1.00 atm of nitrogen gas is mixed with 2.00 atm of hydrogen gas. At equilibrium, the total pressure is 2.00 atm. Calculate the partial pressure of hydrogen gas at equilibrium and calculate the KP value for this reaction. b. Suddenly 2 atm of H2 gas is added to the system. Calculate the partial pressure of each gas after the system reestablishes equilibrium. (Set up the problem, you will find that you need to solve a fourth order polynomial. You can find these roots by using your graphing calculator or use x = 0.4042 or 1.17 to continue to solve the problem.)
3. a. Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia. At 200 °C in a closed container, 1.00 atm of nitrogen gas is mixed with 2.00 atm of hydrogen gas. At equilibrium, the total pressure is 2.00 atm. Calculate the partial pressure of hydrogen gas at equilibrium and calculate the KP value for this reaction.
b. Suddenly 2 atm of H2 gas is added to the system. Calculate the partial pressure of each gas after the system reestablishes equilibrium. (Set up the problem, you will find that you need to solve a fourth order polynomial. You can find these roots by using your graphing calculator or use x = 0.4042 or 1.17 to continue to solve the problem.)
(a)
Given that :
Pressure of nitrogen gas = 1.00 atm
Pressure of hydrogen gas = 2.00 atm
At equilibrium, total pressure = 2.00 atm
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