Question

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.

Answer #1

**Solution:**

a) Given the number of moles = 25.5 moles

=> n = 25.5

Temperature = 283 K

Total pressure = 1 + 0.350 = 1.350 atm

Now Using the ideal gas equation, PV = nRT

=> V = nRT / P

=> V = 25.5 * 8.315 * 283 / 1.350 * 1.013 * 10^5 ( 1 atm = 1.013 * 10^5 Pa)

**=> V = 0.439 m^3 (approx)**

**b)** From the question V2 = 0.5 V1 and P2 = 2
atm

=> P1 * V1 / T1 = P2 * V2 / T2

=> T2 = P2 * V2 * T1 / P1 * V1

=> T2 = 2 * 0.5 * V1 * 283 / 1.350 * V1

=> T2 = 1 * 283 / 1.350

=> T2 = 209.63 K

and in Celcius , it will be 209.63 - 273 = **-63.37
Celcius**

**c)** malar mass of helium = 4 amu

=> Mass = Molar mass * moles

=> Mass = 4 * 25.5

**=> Mass = 102 amu**

please comment for Queries.

Please rate thanks.

.If 17.99 mol of helium gas is at 13.0 ?C and a gauge pressure
of 0.337 atm .
a)Calculate the volume of the helium gas under these
conditions.
b) Calculate the temperature if the gas is compressed to
precisely half the volume at a gauge pressure of 1.05 atm .

If 17.14 mol of helium gas is at 12.9 ∘C and a gauge pressure of
0.387 atm.
a)Calculate the volume of the helium gas under these
conditions.
b) Calculate the temperature if the gas is compressed to
precisely half the volume at a gauge pressure of 1.23 atm.

If 18.74 mol of helium gas is at 11.5 ?C and a gauge pressure of
0.376 atm .
a) Calculate the volume of the helium gas under these
conditions.
b) Calculate the temperature if the gas is compressed to
precisely half the volume at a gauge pressure of 1.17 atm .

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 .

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.

PLEASE ANSWER THESE QUESTIONS. USE UNITS. THANKS IN
ADVANCE
6- If 18.38 mol of helium gas is at 12.1∘C and a gauge
pressure of 0.386 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 1.06
atm .
7- A storage tank contains 21.6 kg of nitrogen (N2) at
an absolute pressure of 3.33 atm ....

A helium-filled toy balloon has a gauge pressure of 0.350 atm
and a volume of 11.0 liters. How much greater is the internal
energy (in J) of the helium in the balloon than it would be at zero
gauge pressure?

4. Three moles of a monatomic ideal gas are initially at a
pressure of 1.00 atm and a temperature of 20.0OC. The gas is
compressed adiabatically to a final pressure of 5.00 atm. Find: (a)
the initial volume of the gas; (b) the final volume of the gas; (c)
the final temperature of the gas; (d) the work done by the gas
during the compression.
Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8
atm-L
Please show...

A sample of helium gas collected at a pressure
of 0.755 atm and a temperature of
281 K is found to occupy a volume of
845 milliliters. How many moles of
He gas are in the sample?

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.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 5 minutes ago

asked 5 minutes ago

asked 14 minutes ago

asked 18 minutes ago

asked 24 minutes ago

asked 41 minutes ago

asked 54 minutes ago

asked 55 minutes ago

asked 55 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago