Question

Consider 4.30 L of a gas at 365 mmHg and 20. ∘C . If the container is compressed to 2.90 L and the temperature is increased to 32 ∘C , what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder.

What pressure would it take to compress 250. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature?

A balloon filled with 2.00 L of helium initially at 1.35 atm of pressure rises into the atmosphere. When the surrounding pressure reaches 310. mmHg, the balloon will burst. If 1 atm = 760. mmHg, what volume will the balloon occupy in the instant before it bursts?

A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90 moles of a gas (n1), and its volume is 50.0 L (V1). If 0.800 mole of gas leak out, and the pressure and temperature remain the same, what is the final volume of the gas inside the cylinder?

A sample of gas in a cylinder as in the example in Part A has an initial volume of 48.0 L , and you have determined that it contains 1.30 moles of gas. The next day you notice that some of the gas has leaked out. The pressure and temperature remain the same, but the volume has changed to 12.0 L . How many moles of gas (n2) remain in the cylinder?

Answer 1

Q1. Consider 4.30 L of a gas at 365 mmHg and 20. ∘C . If the container is compressed to 2.90 L and the temperature is increased to 32 ∘C , what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder.

Apply ideal gas law ratios

P1V1/T1 = P2V2/T2

365*4.30/293 = P*2.90/(32+273)

P = 365*4.30/293 /2.90*(32+273)

P = 563.372 mm Hg

Q2.

What pressure would it take to compress 250. L of helium gas initially at 1.00 atm into a 2.00 L tank at constant temperature?

Apply ideal gas law

P1V1 =P2V2

1*2 = 250*P2

P2 = 0.008 atm