A gas law that describes the pressure, volume, and temperature behavior of a gas sample.

(Pi) (Vi) / Ti = (Pf) (Vf) / Tf , where P is pressure, V is volume, T is Temperature and the subscript (i) is initial & (f) is

final.

7) Use the ideal gas law and calculate the following:

a) The pressure exerted by 2.00 mol of oxygen confined to a volume of 400. mL at 20.0°C.

b) The volume of hydrogen gas in a steel cylinder if 0.525 mol of the gas exerts a pressure of 3.00 atm at a

temperature of 15.0°C.

c) The temperature (in degrees Celsius) of a nitrogen gas sam- ple that has a volume of 2.25 L and a

pressure of 300. torr and contains 0.100 mol.

Ideal Gas Law:

PV = nRT where P, V, and T are defined as they were in the gas laws given earlier. The symbol n stands for the number

of moles of gas in the sample being used, and R is a constant known as the universal gas constant.

Example: Use the ideal gas law to calculate the volume of 0.413 mol of hydrogen gas at a temperature of 20.°C and a

pressure of 1.20 X 10^3 torr.

PV = nRT which would be V = nRT/P if looking for volume as in this example question.

P= 1.20 X 10^3 torr has to be converted to atm so (1.20 X 10^3 torr) (1 atm / 760 torr) = 1.58 atm.

V = ? - Looking for volume according to the question.

n = 0.413 moles

R = 0.0821 L atm / mol k - This is a constant so is always equal to this.

T = 20C + 273 k = 293 k

V = nRT / P = (0.413 moles) (0.0821 L atm/mol k) (293 k) / 1.58 atm

V = 6.29 L

8) A steel cylinder contains a mixture of nitrogen, oxygen, and carbon dioxide gases. The total pressure in the tank

is 2100. torr. The pressure exerted by the nitrogen and oxygen is 810 and 920 torr, respectively.

a) What is the partial pressure in torr of the carbon dioxide in the mixture?

pur-new-sol

Related Questions