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A 642 mL sample of oxygen gas at 23.5°C and 795 mm Hg, is heated to 31.7°C and the volume of the gas expands to 957 mL. What is the new pressure in atm?

A) 0.723 atm
B) 0.932 atm
C) 3.05 atm
D) 5.19 atm

User Anil Arya
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1 Answer

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we can use the combined gas law equation to find the new pressure of the gas.

(P1V1)/(T1) = (P2V2)/(T2)
where P - pressure
V - volume
T - temperature
parameters for the first instance are on the left side and parameters for the second instance are on the right side of the equation
P1 - 795 mm Hg x 0.0013 atm/ mm Hg = 1.033 atm
T1 - 23.5 °C + 273 = 296.5 K
T2 - 31.7 °C + 273 = 304.7 K
substituting the values in the equation

(1.033 atm *642 mL)/(296.5K)= (P*957mL)/(304.7K)
P = 0.712 atm
the answer closest to this value is A) 0.723 atm
therefore answer is
A) 0.723 atm
User Samual
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