1. What is the temperature of 0.53mol of gas at a pressure of 1.1atm and a volum

Question

1. What is the temperature of 0.53mol of gas at a pressure of 1.1atm and a volume of 12.6L ?

2. A cylinder contains 30.0L of oxygen gas at a pressure of 1.9atm and a temperature of 280K . How much gas (in moles) is in the cylinder?

3. Use the molar volume of a gas at STP to calculate the density (in g/L) of carbon dioxide gas at STP.

4. A 1-L flask is filled with 1.15g of argon at 25 ?C. A sample of ethane vapor is added to the same flask until the total pressure is 1.20atm .

a) What is the partial pressure of argon, PAr, in the flask?

b)What is the partial pressure of ethane, Pethane, in the flask?

Explanation / Answer

PV = nRT

1. T = PV/nR = (1.1*12.6)/(0.082*0.53) = 318.91 K = 45.91 C (The R value is taken wrt the units of P, V and n)

2. n = PV/RT = (1.9*30)/(0.082*280) = 2.48 moles

3. density = PM/RT

At STP, P= 1 atm; M= Molar mass of Carbon di oxide= 12 + 2*16= 44 gm ; R=0.082 ; T=273 K

Density = (1*44)/(0.082*273) = 1.966 g/L

4. a) Find moles, using molar mass:

1.15 g argon @ 39.95 g/mol = 0.02879 moles of Argon
T = 25+273 = 298 K
use those moles, to find argon's partial pressure =
Par = nRT/V
Par = (0.02879*0.082*298)/(1) = 0.704 atm

Par = 0.704 atm

b) Total Pressure = Par + Pethane

1.2 = 0.704 + Pethane

Pethane = 1.2-0.704 = 0.496 atm

Pethane = 0.496 atm

(Round off the values according to your need.)

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