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 (*n*1), and its
volume is 50.0 L (*V*1). 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 (*n*2)
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

Part A
Consider 4.30 L of a gas at 365 mmHg and 20. ∘C . If the
container is compressed to 2.70 L and the temperature is increased
to 30. ∘C, what is the new pressure, P2, inside the
container? Assume no change in the amount of gas inside the
cylinder.
Express your answer with the appropriate units.
Part B
A cylinder, with a piston pressing down with a constant
pressure, is filled with 2.00 moles of a gas (n1),...

Consider 4.30 L of a gas at 365 mmHg and 20. ∘C . If the
container is compressed to 2.20 L and the temperature is increased
to 34 ∘C , what is the new pressure, P2, inside the
container? Assume no change in the amount of gas inside the
cylinder.
Express your answer with the appropriate units.

a. A very flexible helium-filled balloon is released from the
ground into the air at 20. ∘C. The initial volume of the balloon is
5.00 L, and the pressure is 760. mmHg. The balloon ascends to an
altitude of 20 km, where the pressure is 76.0 mmHg and the
temperature is −50. ∘C. What is the new volume, V2, of the
balloon in liters, assuming it doesn't break or leak?
b. Consider 4.20
L of a gas at 365 mmHg...

1. scuba diver 40 ft below the ocean surface inhales 45.0 mL of
compressed air from a scuba tank at a pressure of 2.90 atm and a
temperature of 8 ∘ C . What is the final pressure of the air, in
atmospheres, in the lungs when the gas expands to 145.0 mL at a
body temperature of 37 ∘ C , and the amount of gas does not
change?
2. Consider 4.70 L of a gas at 365 mmHg...

A cylinder, with a piston pressing down with a constant
pressure, is filled with 2.00 moles of a gas (n1), and its
volume is 49.0 L (V1). If 0.500 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. A very flexible helium-filled balloon is released from the
ground into the air at 20. ∘C. The initial volume of the balloon is
5.00 L, and the pressure is 760. mmHg. The balloon ascends to an
altitude of 20 km, where the pressure is 76.0 mmHg and the
temperature is −50. ∘C. What is the new volume, V2, of the balloon
in liters, assuming it doesn't break or leak? Express your answer
with the appropriate units.
B. Consider 4.40...

1.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 0.400 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 52.0 L , and you have...

If 3.00 moles of gas in a container has a volume of 60. L and at
a temperature of 400. K, what is the pressure inside the
container?
If 1.9 moles of a gas are held in a container at 5.00 atm and
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What is the mass of 72.6 L of hydrogen gas held at a temperature
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Part A) A certain amount of chlorine gas was placed inside a
cylinder with a movable piston at one end. The initial volume was
3.00 L and the initial pressure of chlorine was 1.40 atm . The
piston was pushed down to change the volume to 1.00 L. Calculate
the final pressure of the gas if the temperature and number of
moles of chlorine remain constant.
part B) In an air-conditioned room at 19.0 ∘C, a spherical
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A weather balloon contains 222 L of He gas at 20. °C and 760.
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1
What volume does 12.5 g of Ar gas at a pressure of 1.05 atm and
a temperature of 322 K occupy? Would the volume be different if the
sample were 12.5 g of He gas under the same conditions?
How many moles...

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