In the fermentation of glucose (wine making),
750 mL of CO2 gas was produced at 37 ∘C and 1.00 atm .
What is the final volume, in liters, of the gas when measured at 24
∘C and 655 mmHg , when n is constant?
First calcule mole of CO2 gas produced
Use ideal gas equation for calculation of mole of gas
Ideal gas equation
PV = nRT where, P = atm pressure= 1.0 atm,
V = volume in Liter = 750 ml = 0.750 L
n = number of mole = ?
R = 0.08205L atm mol-1 K-1 =Proportionality constant = gas constant,
T = Temperature in K = 370C = 273.15+ 37 = 310.15 K
We can write ideal gas equation
n = PV/RT
Substitute the value
n = (1.0 X 0.750)/(0.08205 X 310.15) = 0.029472 mole
now calculte volume of gas at 240C and 655 mm Hg
We know that PV = nRT
V = nRT/P
n = 0.029472mole,
T = 240C = 24+273.15 = 297.15K,
P= 655 mmHg = 0.8615 atm,
R = 0.08205 L atm mol-1 K-1 ( R = gas constant)
V = ?
Substitute these value in above equation.
V = 0.029472 X 0.08205 X 297.15/0.8615 = 0.834 L
Final volue of CO2 gas = 0.834 L
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