# Solved problems on Ideal gas law

Example (1): Calculate the volume of a sample of gas originally occupying 908 mL at 717 torr and 20 oC after its temperature and pressure are changed to 72 oC and 1.07 atm.
Solution
Again, tabulating the data is a good idea.
The volume can be stated in milliliters in both states.
The pressure can be stated in atmospheres in both.
The temperature must be in kelvins in both states; it cannot merely be in the same unit in both states.

Example (2): A 17.3-mL sample of gas originally at standard temperature and pressure is changed to 10.9 mL at 678 torr. Calculate its final temperature in degrees Celsius.
Solution

Example (3): Calculate the volume of 1.63 mol of carbon dioxide gas at 295 K and 1.14 atm.
Solution

Example (4): Calculate the volume of 42.6 g of oxygen gas at 35 oC and 792 torr.
Solution

Because the value of R given previously has units of liters, atmospheres, moles, and kelvins, the data given here are converted to these units:

Example (5): Decide which gas law should be used to solve each of the following:
(a) Calculate the final volume of a sample of gas that has an initial volume of 7.10 L at STP if the temperature and pressure are changed to 33 oC and 696 torr.
(b) Calculate the volume of 0.977 mol of gas at 33 oC and 792 torr.
Solution
(a) The combined gas law can be used.
(b) This problem involves moles and must be solved with the ideal gas law

Example(6): Calculate the volume of 12.7 g of water at 25 oC and 1.00 atm.
Solution
The density of liquid water is 1.00 g/mL, and thus the volume is 12.7 mL.
Not only the laws, but also when to use each one, must be learned.

Example (7): Calculate the pressure of 0.0789 mol of chlorine gas that occupies 891 mL at -15°C.

Solution
The quantities given are converted to the units generally used with the ideal gas law equation.

Note that the nature of the gas is immaterial as long as the number of moles is known.

Example (8): Calculate the number of moles of oxygen gas in a 2.60-L container at 19 oC and 755 torr.

Solution

Example (9): An inflated helium balloon with a volume of 0.55 L at sea level (1.0 atm) is allowed to rise to a height of 6.5 km, where the pressure is about 0.40 atm. Assuming that the temperature remains constant, what is the final volume of the balloon?
solution:
Because n1 = n2 and T1 = T2 ,
which is Boyle’s law. The given information is tabulated:

Example (10): Argon is an inert gas used in light bulbs to retard the vaporization of the tungsten filament. A certain light bulb containing argon at 1.20 atm and 18oC is heated to 85oC at constant volume. Calculate its final pressure (in atm).
Solution:

from combined gas law:
Because n1 = n2 and V1 = V2 , the Equation becomes:
which is Charles’s law. Next we write

Example (11): A small bubble rises from the bottom of a lake, where the temperature and pressure are 8oC and 6.4 atm, to the water’s surface, where the temperature is 25oC and the pressure is 1.0 atm. Calculate the final volume (in mL) of the bubble if its initial volume was 2.1 mL.

Solution:

According to combined gas law Equation:

The given information is summarized:

Reference:
Chemistry / Raymond Chang ,Williams College /(10th edition).
Fundamentals of Chemistry / David E.Goldberg/(5th edition).