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Chemistry
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23 Nov 2019

a. The ammonia produced by reacting .200 mol of nitrogen and .600mol of hydrogen is measured to be 5.00 L at 27 degrees Celsius andone atm. How many moles of nitrogen were used up in thereaction?

b. Using the data in Problem a, calculate the partial pressure ofeach gas in the reaction vessel if all the gases remain in thevessel after the reaction takes place. The temperature of thevessel is 27 degrees Celsius and the pressure in the vessel is 3.0atm.

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4 Mar 2019
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Related questions

Nitrogen gas fills a 300. L reaction container at 100 celsius and 1.00 atm.

a) WHat is the density of nitrogen gas?

b) Determine the volume of the same quanity of nitrogen at 0 celsius and 1.25 atm.

c) what would be the pressure of an equal mass of argon in the same vessel at 100 celsius?

d) How many moles of nitrogen need to be removed if the pressure is to remain at 1.00 atm when the container is heated to 150 Celsius.

Thankyou in advance and please show works.

1.calculare the final pressure of 0.8 g of hydrogen gas (H2) when stored in 20 L container at 27 degree Celsius.
2.What is the final volume of 0.3 moles of a gas which occupies 4.5 L at 27 degree Celsius when it is heated up to 47 degree Celsius under constant pressure?
3.A gas is stored under 2 atm,what is the final volume of a gas if the pressure was halved under constant temperature?
4.calculate the density of SO2 gas at STP.
5.Calculate the density of CH4 gas at 1.5 atm and 15 degree Celsius.

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 1.00 atm. Assume the temperature is constant and that the reaction goes to completion.  

  1. Calculate the partial pressure of ammonia in the container after the reaction has reached completion.
  2. Calculate the volume of the container after the reaction has reached completion.

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