Asked by Jake
Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200
oC in a closed
container, 1.1 atm of nitrogen gas is mixed with 2.1 atm of hydrogen gas in an otherwise empty container.
At equilibrium, the total pressure is 2.2 atm. Calculate the partial pressure of hydrogen gas at equilibrium.
oC in a closed
container, 1.1 atm of nitrogen gas is mixed with 2.1 atm of hydrogen gas in an otherwise empty container.
At equilibrium, the total pressure is 2.2 atm. Calculate the partial pressure of hydrogen gas at equilibrium.
Answers
Answered by
DrBob222
Is there a Kp? Kc?
Answered by
Jake
there isnt a kp or a kc
Answered by
DrBob222
Try this.
..........N2 + 3H2 ==> 2NH3
initial...1.1..2.1......0
change...-x....-3x......2x
equil...1.1-x..2.1-3x...2x
Ptotal = 2.2 = 1.1-x+2.1-3x+2x
Solve for x and substitute into 2.1-3x for pH2. Something like 0.6 atm. for pH2.
..........N2 + 3H2 ==> 2NH3
initial...1.1..2.1......0
change...-x....-3x......2x
equil...1.1-x..2.1-3x...2x
Ptotal = 2.2 = 1.1-x+2.1-3x+2x
Solve for x and substitute into 2.1-3x for pH2. Something like 0.6 atm. for pH2.
Answered by
Jake
Thanks it worked perfectly
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