If 7.54 moles of an ideal gas has a pressure of 3.95 atm, and a volume of 66.93
ID: 1010759 • Letter: I
Question
If 7.54 moles of an ideal gas has a pressure of 3.95 atm, and a volume of 66.93 L, what is the temperature of the sample in degrees Celsius?
An ideal gas in a sealed container has an initial volume of 2.65 L. At constant pressure, it is cooled to 18.00 °C where its final volume is 1.75 L. What was the initial temperature?
2.35 g of an unknown gas at 27 °C and 1.05 atm is stored in a 1.85-L flask.What is the molar mass of the gas? What is the molar mass of the gas?
The combustion of octane, C8H18, proceeds according to the reaction If 354 mol of octane combusts, what volume of carbon dioxide is produced at 28.0 °C and 0.995 atm?
Explanation / Answer
1. PV = nRT
P = 3.95atm
V = 66.93L
n = 7.54 moles
T = PV/nR
= 3.95*66.93/7.54*0.0821 = 427K = 427-273 = 154C0 >>>>> answer
2. initial final
T1 = T2 = 18C0 = 18+273 = 291K
V1 = 2.65L V2 = 1.75L
V1/T1 = V2/T2
T1 = V1T2/V2
= 2.65*291/1.75 = 440K = 440-273 = 167C0
3. PV = nRT
n = W/M
PV = WRT/M
M = WRT/PV
W = 2.35g
R = 0.0821L-atm/mole-K
T = 27C0 = 27+273 = 300K
P = 1.05atm
V = 1.85L
M = WRT/PV
= 2.35*0.0821*300/1.05*1.85 = 29.8g/mole
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