Question

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 and 20. ∘C . If the
container is compressed to 3.00 L and the temperature is increased
to 31 ∘C , what is the new pressure, *P*2 , inside the
container? Assume no change in the amount of gas inside the
cylinder.

3. 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 0.400 mole of gas leak out,
and the pressure and temperature remain the same, what is the final
volume of the gas inside the cylinder?

4.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 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 13.0 L . How many moles of gas
(*n*2 ) remain in the cylinder?

Answer #1

**1)**

**Given:**

**Pi = 2.90 atm**

**Vi = 45.0 mL**

**Vf = 145.0 mL**

**Ti = 8.0 oC**

**= (8.0+273) K**

**= 281 K**

**Tf = 37.0 oC**

**= (37.0+273) K**

**= 310 K**

**use:**

**(Pi*Vi)/(Ti) = (Pf*Vf)/(Tf)**

**(2.9 atm*45 mL)/(281.0 K) = (Pf*145.0 mL)/(310
K)**

**Pf = 0.993 atm**

**Answer: 0.993 atm**

**2)**

**Given:**

**Pi = 365 mmHg**

**Vi = 4.70 L**

**Vf = 3.00 L**

**Ti = 20.0 oC**

**= (20.0+273) K**

**= 293 K**

**Tf = 31.0 oC**

**= (31.0+273) K**

**= 304 K**

**use:**

**(Pi*Vi)/(Ti) = (Pf*Vf)/(Tf)**

**(365.0 mmHg*4.7 L)/(293.0 K) = (Pf*3.0 L)/(304.0
K)**

**Pf = 593 mmHg**

**Answer: 593 mmHg**

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...

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 2.90 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...

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?

Typically, when a person coughs, he or she first inhales about
2.30 L of air at 1.00 atm and 25 ∘C. The epiglottis and the vocal
cords then shut, trapping the air in the lungs, where it is warmed
to 37 ∘C and compressed to a volume of about 1.70 L by the action
of the diaphragm and chest muscles. The sudden opening of the
epiglottis and vocal cords releases this air explosively. Just
prior to this release, what is...

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...

Part A)
If the sample is compressed to a volume of 15.4 L , what is its
pressure?
Express the pressure in atmospheres to three significant
figures.
Part B) A syringe containing 1.30 mL of oxygen gas is cooled
from 97.1 ∘C to 0.4 ∘C. What is the final volume Vf of
oxygen gas?
Part C)
What is its volume after an additional 0.26 mol of gas is added
to the cylinder? (Assume constant temperature and pressure.)
Express your answer...

1) A scuba diver swims below the surface, breathing air from
tanks of her scuba gear.
a. It’s easiest for her to maintain a constant depth if the
buoyant force on her and her equipment exactly balances their
weight. How should her average density compare with that of the
water around her?
b. When she is 20 m below the surface of the water, what is the
pressure pushing inward on her chest?
c. When she breathes, she expects air...

1. 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 1.20 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? Express your answer with the
appropriate units....

All pressure–volume–temperature relationships for gases can be
combined into a single relationship known as the combined gas
law. This expression can be used when looking at the effect of
changes in two of these variables on the third as long as the
amount of gas (number of moles) remains constant. To use the
combined gas law properly, you must always express the temperatures
in kelvins. The combined gas law can be represented as follows:
P1V1/T1=P2V2/T2
1.)
A very flexible helium-filled...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 3 minutes ago

asked 3 minutes ago

asked 4 minutes ago

asked 5 minutes ago

asked 16 minutes ago

asked 22 minutes ago

asked 26 minutes ago

asked 28 minutes ago

asked 37 minutes ago

asked 43 minutes ago

asked 49 minutes ago

asked 49 minutes ago