Question #ddb73

1 Answer
Mar 6, 2014

This is a gas law stoichiometry problem because you are in conditions other than STP.

Begin by determining how many moles of #CO_2# you can theoretically produce based upon stoichiometry.

43.0 g #CH_4# / 16 g #CH_4# = 2.687 moles #CH_4#
(16 g is the molar mass of #CH_4#)

Convert moles #CH_4# to moles #CO_2# using the mole ratio from the balanced chemical equation.

2.687 moles #CH_4# x 1 mole #CO_2# / 1 mole #CH_4# = 2.687 moles #CO_2#

Now use the moles in the ideal gas law to convert to volume at non STP values for temperature and pressure.

P = 795 mmHg / 760 mmhg = 1.04 atm
V = ???
n = 2.687 moles #CO_2#
R = 0.0821 atm L/mole K
T = 85 C + 273 = 358 K

PV = nRT converts to v = nrt/P

V = 2.687 moles (0.0821 atm L/mole K) ( 358 K) / 1.04 atm.
all units cancel except Liters (L)

V = 75.9 L #CO_2#

I hope this was helpful.
SMARTERTEACHER