Question

2.50 Liters of CO2 gas (ideal) at 25^{\circ }C and 1.o atm of pressure is allowed to expand in volume until the final pressure and temperature are 0.50 atm and 15^{\circ }C , respectively:

a) Calculate the final volume of the gas.

b) Calculate the # of moles, n, of the gas.

c) Calculate the # of grams of the gas.

Answer #1

**Initially P1 = 1 atm , V1 = 2.5 L
, T1 = 25C = 25+273 = 298 K**

**final P2 = 0.5 atm , T2 = 15C = 15+273 = 288
K**

**we find moles of gas using PV =
nRT equation using initial
conditions**

**where R = gas constant = 0.08206 liter
atm/molK**

**b) 1 atm x 2.5 liter = n x 0.08206 liter atm/molK x 298
K**

**n = 0.10223**

**a) now using moles we calculate final volume since P , T
, V changed but not moles as gas is not added or
removed.**

**0.5 atm x V = 0.10223 mol x 0.08206 liter atm/molK x 288
K**

**V = 4.83 L**

**c) CO2 moles = 0.10223**

**CO2 mass = Moles x molar mass of
CO2
( molar mass of CO2 = 44 g/mol)**

**hence mass = 0.10223 x 44 g/mol**

**
= 4.5 g**

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