A scientist is examining a mixture of nitrogen, hydrogen, and ammonia. The individual pressures that are exerted by nitrogen and hydrogen are 0.26 atm and 0.28 atm, respectively. If the total pressure is 0.90 atm, what is the partial pressure of ammonia?
Answers
A scientist is examining a mixture of nitrogen, hydrogen, and ammonia. The individual pressures that are exerted by nitrogen and hydrogen are 0.26 atm and 0.28 atm, respectively. If the total pressure is 0.90 atm, what is the partial pressure of ammonia?Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia gas (NH3). You have nitrogen and hydrogen gases in a 15.0 L container fitted with a movable piston (the piston allows the container volume to change so as to keep the pressure constant inside the container). Initially the partial pressure of each reactant gas is 2.73 atm. Assume the temperature is constant and the reaction goes to completion.
Chemistry Partial Pressure
Answer:
The partial pressure of ammonia is 1.82 atm. The new volume is 10.0 L.
Explanation:
Step 1: Identify the limiting reactant
We can use partial pressures as a replacement for moles because P∝n.
mmmmmmN2m+m3H2→2NH3
P(atm):mll2.73mmm2.73
Divide by:mll1mmmml3
Moles rxn:ll2.73mmm0.910
Hydrogen is the limiting reactant because it gives the fewest moles of reaction,
Step 2: Calculate the partial pressures after the reaction
mmmmmmN2m+m3H2→2NH3
I:/atm:mlm2.73mmm2.73mmll0
C:/atm:ml-0.910mml-2.73ml+1.82
E:/atm:mm1.82mmmm0mmll1.82
The product mixture will contain ammonia and unreacted nitrogen, each with a partial pressure of 1.82 atm.
Ptotal=PN₂+PNH₃=1.82 atm + 1.82 atm=3.64 atm
PNH