This question concerns the ideal gas law.

Question

Determine the temperature of 0.105 moles of gas in a volume of 1750 mL at 15.0 bar. State your answer in degrees Fahrenheit.

Answer 1

The ideal gas law is PV = nRT

P = pressure (units of atm, bar, torr, etc.) = 15.0 bar x 0.9869 atm / bar = 14.80 atm

V = volume in liters = 1750 ml x 1 L / 1000 ml = 1.750 L

n = moles = 0.105 mols

R = gas constant (units must match those for pressure) = 0.0821 Latm/Kmol

T = temperature in Kelvin = ?

Solving for T, we have...

T = PV / nR = (14.80 atm)(1.75 L) / (0.105 mol)(0.0821 Latm/Kmol)

T = 3004 K

Converting this to Fahrenheit, we have...

ºF = (K - 273.15) x 1.8 + 32

ºF = (3004 - 273.15) x 1.8 + 32

ºF = 4948ºF = 4950ºF (3 sig.figs.)