Question

Helium gas with a volume of 2.60 L , under a pressure of 0.160 atm and at a temperature of 43.0 ∘C, is warmed until both pressure and volume are doubled.

Part A

What is the final temperature?

Express your answer using three significant figures.

Part B

How many grams of helium are there? The molar mass of helium is 4.00 g/mol.

Answer #1

1. A sample of gas with an initial volume of 28.2 L at a
pressure of 728 mmHg and a temperature of 301 K is compressed to a
volume of 14.9 L and warmed to a temperature of 375 K. What is the
final pressure of the gas?
2. A gas sample with a volume of 5.3 L has a pressure of 725
mmHg at 24C. What is the pressure of the sample if the volume
remains at 5.3 L...

1a. A sample of methane gas at 292 K and 0.160 atm occupies a
volume of 2.06 L. If the pressure of the gas is increased, while at
the same time it is heated to a higher temperature, the final gas
volume
a. will be smaller than 2.06 L.
b. will be larger than 2.06 L.
c. could be larger or smaller than 2.06 L depending on the final
pressure and temperature.
1b. A sample of oxygen gas at 300...

A) A syringe containing 1.25 mL of oxygen gas is cooled from
90.3 ∘C to 0.9 ∘C. What is the final volume Vf of oxygen
gas?
B) What is its volume after an
additional 0.30 mol of gas is added to the cylinder? (Assume
constant temperature and pressure.) Express your answer to three significant
figures.
C) What is the pressure in a 12.9
L cylinder filled with 0.425 mol of nitrogen gas at a temperature
of 300 K ?
D)...

A sample of helium gas has a volume of 5.10 L at a pressure of
815 mmHg and a temperature of 26 ∘C.
A) What is the pressure of the gas in atm when the volume and
temperature of the gas sample are changed to 1610 mLand 338 K if
the amount of gas is constant?
B) What is the pressure of the gas in atm when the volume and
temperature of the gas sample are changed to 2.33 L...

If 15.82 mol of helium gas is at 12.4 ∘C and a gauge pressure of
0.339 atm .
Part A: Calculate the volume of the helium gas under these
conditions.
Part B: Calculate the temperature if the gas is compressed to
precisely half the volume at a gauge pressure of 1.19 atm.

25.5 moles of helium gas is at 10 0C and gauge pressure of
0.350 ATM. Calculate
a) the volume of the helium (He) gas under these
conditions;
b) the temperature of the gas when it is compressed to
precisely half of the original volume at the gauge pressure of 1.00
ATM;
c) the mass of the helium gas.

Part A
A mixture of He, Ar, and Xe has a total pressure of 2.90 atm .
The partial pressure of He is 0.450 atm , and the partial pressure
of Ar is 0.250 atm . What is the partial pressure of Xe? Express
your answer to three significant figures and include the
appropriate units.
Part B
A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250
mole O2 , and an unknown quantity of He....

Part A
A mixture of He, Ar, and Xe has a total pressure of 2.20 atm .
The partial pressure of He is 0.450 atm , and the partial pressure
of Ar is 0.400 atm . What is the partial pressure of Xe? Express
your answer to three significant figures and include the
appropriate units.
Part B
A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250
mole O2 , and an unknown quantity of He....

Charles's Law
A sample of helium gas at a pressure of 0.905 atm and a temperature
of 230°C, occupies a volume of 615mL. If the gas is cooled at
constant pressure until it's volume is 523mL, the temperature of
the gas sample will be ____°C
A sample of oxygen gas at a pressure of 960 mm Hg and
a temperature of 81°C, occupies a volume of 14.9 liters. I the gas
is heated at constant pressure at a temperature of...

If 17.05 mol of helium gas is at 12.2 ∘C and a gauge pressure of
0.314 atm . Calculate the volume of the helium gas under these
conditions. Calculate the temperature if the gas is compressed to
precisely half the volume at a gauge pressure of 1.05 atm .

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 18 minutes ago

asked 22 minutes ago

asked 30 minutes ago

asked 31 minutes ago

asked 36 minutes ago

asked 45 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago