Calculate each of the following quantities for an ideal gas. Part A Calculate th

Question

Calculate each of the following quantities for an ideal gas.

Part A

Calculate the volume of the gas, in liters, if 1.70 mol has a pressure of 1.21 atm at a temperature of -5 C.

Express the volume in liters to three significant digits.

Part B

Calculate the absolute temperature of the gas at which 3.53×103 mol occupies 448 mL at 755 torr .

Express the temperature in kelvins to three significant digits.

Part C

Calculate the pressure, in atmospheres, if 2.55×103 mol occupies 413 mL at 139 C.

Express the pressure in atmospheres to three significant digits.

Part D

Calculate the quantity of gas, in moles, if 126 L at 50.0 C has a pressure of 11.35 kPa .

Express the amount in moles to three significant digits.

Explanation / Answer

We would be using the relation for ideal gas,

PV = nRT

Part A. Calculate the volume of the gas, in liters, if 1.70 mol has a pressure of 1.21 atm at a temperature of -5 C

Given.

n = 1.70 mols

P = 1.21 atm

Temperature = -5oC = 273 - 5 = 268 K

R = 0.08206 L.atm/mol.K

Feed the values,

V = 1.70 x 0.08206 x 268 / 1.21 = 30.898 L = 30.9L [three significant figures]

Part B. Calculate the absolute temperature of the gas at which 3.53×103 mol occupies 448 mL at 755 torr

n = 3.53×103 mol

P = 755 torr = 0.99342 atm

V = 448 mL = 0.448 L

Feed the values,

T = 0.99342 x 0.448 / 3.53×103 x 0.08206 = 1536.401 K = 1540K [three significant figures]

Part C. Calculate the pressure, in atmospheres, if 2.55×103 mol occupies 413 mL at 139 C.

n = 2.55×103 mol

V = 413 mL = 0.413 L

T = 139 C = 139 + 273 = 412 K

Feed the values,

P = 2.55×103 x 412 x 0.08206 / 0.413 = 0.209 atm [three significant figures]

Part D. Calculate the quantity of gas, in moles, if 126 L at 50.0 C has a pressure of 11.35 kPa

P = 11.35 kPa = 0.112 atm

T = 50 oC = 50 + 273 = 323 K

V = 126 L

Feed the values,

n = 0.112 x 126 / 0.08206 x 323 = 0.532 mol [three significant figures]

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