Butane and oxygen were allowed to completely react at 540 torr and 298 K. After
the exothermic reaction, 620 L of CO2 was collected at 823 K and 750 torr. How
many liters of O2 gas at 540 torr and 298 K were consumed?
2 C, H10 (8) + 13 0,(8) →800,() + 10 H2O(g)

510 L of oxygen gas were consumed.

Explanation:

According to ideal gas equation:

P = pressure of gas = 750 torr = 0.99 atm   (760 torr= 1atm)

V = Volume of gas = 620 L

n = number of moles of carbon dioxide = ?

R = gas constant =

T =temperature =

According to stoichiometry:

8 moles of are produced by = 13 moles of oxygen

Thus 9.08 moles of are produced by = moles of oxygen

P = pressure of gas = 540 torr = 0.71 atm   (760 torr= 1atm)

V = Volume of gas = ?

n = number of moles of oxygen = 14.8

R = gas constant =

T =temperature =

Thus 510 L of oxygen gas were consumed.

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