Will mark as brainliest. 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

Where, P is the pressure of the gas, V is volume of the gas and T is the temperature of the gas in Kelvin.
For two situations, we can use that as,P₁V₁/T₁= P₂V₂/T₂
P₁ = 795 mm HgV₁ =  642 mLT₁ = (273 + 23.5) K = 296.5 KP₂ = ? V₂ = 957 mLT₂ = (273 + 31.7) K = 304.7 K
By applying the formula,
795 mm Hg x 642 mL / 296.5 K = P₂ x 957 mL / 304.7 K                                              P₂ = 548.07 mm Hg                                              P₂ = 548 mm Hg760 mmHg = 1 atm548 mm Hg = 1 atm x (548 mmHg / 760 mmHg) = 0.721 atm
Pressure of gas = 548 mm Hg = 0.721 atm

About 8 gallons of fuel will be used. (8.08)