Four hundred grams of nitrogen gas (molecular weight=28g/mole) are stored in a 10-liter container. Set up an excel worksheet to determine the pressure of the gas (in atmospheres) as a function of temperature and volume, assuming nitrogen is an ideal gas. Place value of each variable in its own cell. Label all of the quantities clearly. Recall that the ideal gas law is PV=nRT where P=pressure(atmospheres) V=volume(liters) n=number of moles (mass of gas/molecular weight) R= ideal gas constant (.082054 liter atm/mole K) T= absolute temperature (degrees K= degrees celcius +273) (a) what presssure corresponds to a temperature of 22 degrees celcius? (b) what is the pressure if the temperature is changed to 37 degrees celcius? (c ) what is the pressure if the original temperature (22 degrees Celcius) is restored but the volume of the container is reduced to 7 liters? (d) what is the pressure if the original 10-liter container contains 300 grams of oxygen (molecular weight=32 g/mole) at 18 degrees celcius?

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