Initially, a 55.0 liter compressible container, holding 2.4 moles of a gas, exerts a pressure of 760 millimeters of mercury at a temperature of 280 Kelvin. What is the pressure when the container is compressed to 43.0 liters, the moles of gas reduces to 1.8 moles, and the temperature changes to 36 degrees Celsius?
Answer

93.7 mm Hg

492 mm Hg

740 mm Hg

805 mm Hg

Question

Initially, a 55.0 liter compressible container, holding 2.4 moles of a gas, exerts a pressure of 760 millimeters of mercury at a temperature of 280 Kelvin. What is the pressure when the container is compressed to 43.0 liters, the moles of gas reduces to 1.8 moles, and the temperature changes to 36 degrees Celsius?
Answer
		
93.7 mm Hg
		
492 mm Hg
		
740 mm Hg
		
805 mm Hg

aaronq · Answer

use the ideal gas law, PV=nRT, with the conditions specified.

V=43.0 L, n=1.8 moles, T= 36 degrees Celsius (needs to be in Kelvin)