A quantity of N2 gas originally held at 3.80 atm pressure in a 1.00 L container...
A quantity of N2 gas originally held at 3.80 atm pressure in a 1.00 L container at 26.0ºC is transferred to a 10.0 L container at 20.0ºC. A quantity of O2 gas originally at 4.75 atm and 26.0ºC in a 5.00 L container is added to the 10.0 L container already containing the N2.
a) Draw a diagram outlining this experiment, labeling the various quantities.
b) Calculate the total pressure in the new container.
c) What is the mole fraction of the nitrogen gas in the newly formed mixture?
Homework Answers
In the above image there is IDEAL GAS equation
- Pressure(P) in atms.
- Volume(V) in Litres.
- n is the number of gas in the container.
- R is ideal gas constant. R = 0.0821.
- Temperature(T) is in Kelvin. For conversion T(in K) = T(in C) + 273.
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