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Ideal Gas
Thermodynamics
100
A sample of argon gas at STP occupies 56.2 liters. Determine the number of moles of argon and the mass in the sample. (1 atm, 0C)
n = PV / RT n = [ (1.00 atm) (56.2 L) ] / [ (0.08206 L atm mol¯1 K¯1) (273.0 K) ] n = 2.50866 mol g = 100 g
100
q = mcΔT q = (25 g)x(4.18 J/g·°C)x(100 °C) q = 10450 J
What is the heat in Joules required to raise the temperature of 25 grams of water from 0 °C to 100 °C? What is the heat in calories? Cs =4.18 J/g C
200
T = PV / nR T = (1.95 atm) (12.30 L) / (0.654 mol) (0.0821) T = 447 K
At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 atmospheres?
300
n = PV / RT n = [ (.92atm) (48.0 L) / (0.0821) (293.0 K) n = 1.8388 mol 96.0 g / 1.8388 mol = 52.2 g/mol
96.0 g. of a gas occupies 48.0 L at 700.0 mm Hg and 20.0 °C. What is its molecular weight?
400
n = PV/RT --> (1Atm)(22.414L)/(.0821)(273) = 1 mm = g/mol --> 30.6g/1mol --> 30.6 g/mol
A 30.6 g sample of gas occupies 22.414 L at STP. What is the molecular weight of this gas?
500
P = nRT/V 5.600 g / 44.009 g/mol = 0.1272467 mol p = (0.1272467 mol) (0.0821) (300 K) / (.4L) P = 0.7831 atm
5.600 g of solid CO2 is put in an empty sealed 4.00 L container at a temperature of 300 K. When all the solid CO2 becomes gas, what will be the pressure in the container?