A sample of argon gas has a volume of 735 mL at a pressure of 1.40 atm and a tem

Question

A sample of argon gas has a volume of 735 mL at a pressure of 1.40 atm and a temperature of 104 C. (A) What is the volume of the gas in milliliters when the pressure and temperature of the gas sample are changed to 658 mmHg and 309 K ? (B) What is the volume of the gas in milliliters when the pressure and temperature of the gas sample are changed to 0.800 atm and 74 C? (C) What is the volume of the gas in milliliters when the pressure and temperature of the gas sample are changed to 16.8 atm and -23 C?

Explanation / Answer

Using the ideal gas law , pv = nRT

where p is pressure , v is volume , n is no. of moles , R is universal gas constant and T is temperature in kelvin.

A) pv = nRT

1.40 x 0.735 = n x 0.0821 x 377.15

n = 0.033 moles

Now using this n ,

pv = nRT

658 mmHg = 0.86579 atm

0.86579 x v = 0.033 x 0.0821 x 309

v = 972.8mL

B)

pv = nRT

0.800 x V = 0.033 x 0.0821 x 347.15

V = 1182.8 mL

C)

pv = nRT

16.8 x V = 0.033 x 0.0821 x 250.15

V = 40.58 mL

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