13.4 Review Name______
The Ideal Gas Law : PV = nRTR = 0.0821 atm-L/mol-K
Fill in the blank: Complete the following sentences by circling the correct choice.
1)Real gases behave like ideal gases except at very ( high or low ) temperatures.
2)The gas constant, R , is equal to 0.0821 when the pressure is expressed in ( kPa or atm )
3)As more gas particles are added to a container, there are ( more or less ) collisions because the particles don’t go as far.
4)The number of moles of a gas is ( inversely or directly ) proportional to its volume at STP.
5)Real gases behave like ideal gases except at very ( high or low ) pressure.
6)At a constant temperature, the pressure exerted by one mole of a gas ( decreases or increases ) if the volume available is increased.
7)The ideal gas equation will only give the correct values if the temperature is expressed in ( oC or K ).
Use the ideal gas equation to calculate the unknown value(s) for each row. Write your answers in the table.
Pressure / Temperature / # moles / R / Volume1.02 atm / 300K / 0.821 mol / 0.0821
762 mmHg / 2.16 mol / 0.0821 / 48.3 L
101.325 kPa / 0oC / 0.0821 / 22.4 L
20oC / .038 mol / 0.0821 / 6.76 L
Matching: Match each variable in the ideal gas equation listed on the left with the appropriate unit of measurement. You may write one or more letters on each line.
8)______number of moles
9)______volume
10)______pressure
11)______temperature
12)Explain the relationship between temperature and pressure.
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Problems: Solve each of the following problems as directed. Show all of your work!
13)If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?
14)Calculate how many grams of methane (CH4) are in a sealed 800 mL flask at room temperature (22oC) and 780 mm Hg of pressure.
15)If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87oC, how many moles of gas do I have?
16)The atmospheric pressure on Mars is about 6.75 millibars (1 bar = 100 kPa = 0.9869 atm), and the nighttime temperature can be about -75°C on the same day that the daytime temperature goes up to 8°C. What volume would a bag containing 1.00 g of H2 gas have at both the daytime and nighttime temperatures
17)A volume of 26.5 mL of nitrogen gas was collected in a tube at a temperature of 17° C and a pressure of 737 mm Hg. The next day the volume of the nitrogen was 27.1 mL with the barometer still reading 737 mm Hg. What was the temperature on the second day?