Question

You may use any of the following values of the ideal gas constant R to solve the problems: R = 0.082057 Lam mol R=0.083145 L bar mol R = 62 364 Tort mol K 15 230 1. Calculate the moles of gas in 64.21 mL oxygen at 22.3 °C and 0.9531 bar. 62.364064 0.9331). (295.45) 2. Calculate the absolute temperature of 0.01937 mol hydrogen at 121.7 Torr and 4.137 L. 3. Calculate the volume, in liters, of 1.000 mol argon at -191 °C and 0.315 atm. 4. Calculate the pressure exerted by 192 mol of carbon dioxide at 25 °C and 2.50 L. 5. Calculate the mass of helium gas for a 180.0 L cylinder at a pressure of 155 atm and 25.0 *C. Revised 12/15/2014 1 of 1

Answer 1

We will use ideal gas equation for each questions;

PV = nRT

Where P is pressure in atm, V is volume in liters, n is moles, R is gas constant and T is temperature in Kelvin.

Moles (n) = mass / molar mass

1)

PV = nRT

n = PV / RT = 0.9531*0.06421 / 0.083145 * (22.3+273)

n = 0.002492 moles ....Answer

2)

T = PV/nR = 121.7*4.137 / 0.01937*62.364

T = 416.785 K ...Answer

3)

V = nRT/P = 1 * 0.082057 * (273-191) / 0.315

V = 21.36 liters ...Answers

4) this can be calculated in same way as above

5)

n = PV/RT = 155*180/0.082057*(25+273)

n = 1140.965 moles

Mass of Helium = moles * molar mass = 1140.965 * 4 = 4563.86 grams ...Answer

Let me know if any doubts/answer is not matching.