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?

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?
		
1.1 x 103 mm Hg
		
1.4 x 103 mm Hg
		
1.5 x 102 mm Hg
		
3.9 x 102 mm Hg

anonymous · Answer

you first need to find molar mass then continue to multiply by the numbers given and round to the nearest tenth

abb0t · Answer

Yes, get the moles, then use $\sf \color{violet}{PV=nRT}$, rearrange, and solve for $\sf \color{red}{P}$
P = pressure
V = volume
n = moles
R = gas constant 
T = temp