Ammonia (NH3) reacts with molecular oxygen as 4 NH3(g) + 5 O2 (g) → 4 NO(g) + 6 H₂O (g) Initially NH3 and O₂ are separated as shown here. When the valve (the X) is opened, the reaction quickly goes to completion. Assume that the temperature is constant at 25°C. X NH3 0₂ 3.0 L at 4.0 L at 0.500 atm 0.700 atm (a) Determine what gases remain at the end of the reaction and calculate how many moles of each gas remain. (b) Calculate the mole fraction of the remaining gases. (c) If the total pressure in the container at the end of the reaction is 0.650 atm, calculate the partial pressure of each remaining gas.

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Chapter1: Chemical Foundations
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Ammonia (NH3) reacts with molecular oxygen as
4 NH3(g) + 5 O2 (g) → 4 NO(g) + 6 H₂O (g)
Initially NH3 and O₂ are separated as shown here. When the valve (the X) is opened, the
reaction quickly goes to completion. Assume that the temperature is constant at 25°C.
NH3
X
0₂
3.0 L at
4.0 L at
0.500 atm
0.700 atm
(a) Determine what gases remain at the end of the reaction and calculate how many moles
of each gas remain.
(b) Calculate the mole fraction of the remaining gases.
(c) If the total pressure in the container at the end of the reaction is 0.650 atm, calculate
the partial pressure of each remaining gas.
Transcribed Image Text:Ammonia (NH3) reacts with molecular oxygen as 4 NH3(g) + 5 O2 (g) → 4 NO(g) + 6 H₂O (g) Initially NH3 and O₂ are separated as shown here. When the valve (the X) is opened, the reaction quickly goes to completion. Assume that the temperature is constant at 25°C. NH3 X 0₂ 3.0 L at 4.0 L at 0.500 atm 0.700 atm (a) Determine what gases remain at the end of the reaction and calculate how many moles of each gas remain. (b) Calculate the mole fraction of the remaining gases. (c) If the total pressure in the container at the end of the reaction is 0.650 atm, calculate the partial pressure of each remaining gas.
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