Initially, a 1.50-liter compressible container of 0.35 moles of a gas exerts a pressure of 740 millimeters of mercury at a temperature of 275 Kelvin. What is the pressure when the container is compressed to 0.50 liters, the moles of gas reduces to 0.20 moles, and the temperature changes to 32 degrees Celsius?
Answer

1.1 x 103 mm Hg

1.4 x 103 mm Hg

1.5 x 102 mm Hg

3.9 x 102 mm Hg

Question

Initially, a 1.50-liter compressible container of 0.35 moles of a gas exerts a pressure of 740 millimeters of mercury at a temperature of 275 Kelvin. What is the pressure when the container is compressed to 0.50 liters, the moles of gas reduces to 0.20 moles, and the temperature changes to 32 degrees Celsius?
Answer
		
1.1 x 103 mm Hg
		
1.4 x 103 mm Hg
		
1.5 x 102 mm Hg
		
3.9 x 102 mm Hg

abb0t · Answer

Use the PV=nRT equation.

abb0t · Answer

solve for P (pressure)

anonymous · Answer

I am not sure how could you help me through it please

anonymous · Answer

PX0.5 = 0.2 X R X (32 + 273)
Therefore P = 0.2X0.0821X305/0.5
P = 10.02 atm
1 atm = 760 mm Hg
So 10.02 atm  = 7615.2 mm Hg

Unfortunately the options dont seem to match.