1.Calculate the density of nitrogen gas (in g/L) at 939 mm Hg and 50.7 °C. 2.A 1

Question

1.Calculate the density of nitrogen gas (in g/L) at 939 mm Hg and 50.7 °C.

2.A 1.15-g sample of an unknown gas has a volume of 869 mL and a pressure of 551 mm Hg at 41.5 °C. Calculate the molar mass of this compound.

3.A sample of Ne gas has a volume of 554 mL, has a pressure of 595 mm Hg, and is at a temperature of 26.1 °C. Calculate the amount (in moles) of Ne in the gas sample.

4.A 7.01-L sample of gas has a pressure of 1.71 atm and a temperature of 83 °C. The sample is compressed to a volume of 4.93 L and is heated to 140 °C. Calculate the new pressure of the gas, assuming that no gas escaped during the experiment.

Explanation / Answer

PV = nRT

where:

P is the pressure of the gas

V is the volume of the gas

n is the amount of substance of gas (in moles)

R is gas constant = = 0.0821 L atm K-1 Mol-1

T is the absolute temperature of the gas.

Question 2

P = 551 mmHg or 0.725 atm

V= 869 ml or 0.869 liter

T = 41.5 +273 = 314.5 K

0.725 x 0.869 = n x 0.0821x 314.5

n = 0.0244 Moles

Molar mass of the compound = 1.15 g /0.0244 mole = 47.13 g/mol

Question 3

P = 595 mmHg or 0.78289 atm

V = 0.554 Liter

T = 26.1+273 = 299.1 K

0.78289 x 0.554 = n x 0.0821 x 299.1

n = 0.01766 Moles

0.01766 Moles of Ne gas is present.

Quesiton 4

V = 7.01

P = 1.71 atm

T = 273 + 83 = 356 K

7.01 x 1.71 = n x 0.0821 x 356

n = 0.410 Moles

using the moles we can calculate the new pressure

P x 4.93 = 0.410 x 0.0821 x 413

P = 2.82 atm

New pressure is 2.82 atm

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