Question

A balloon is floating around outside your window. The temperature outside is -13 ∘C , and the air pressure is 0.800 atm . Your neighbor, who released the balloon, tells you that he filled it with 3.00 moles of gas. What is the volume of gas inside this balloon?

Answer 1

Answer:

80.0 L

Explanation:

Given data

• Pressure (P): 0.800 atm

• Volume (V): ?

• Number of moles (n): 3.00 mol

• Ideal gas constant (R): 0.0821 atm.L/mol.K

• Temperature (T): - 13°C + 273.15 = 260 K

We can find the volume of the gas inside the balloon using the ideal gas law.

P × V = n × R × T

V = n × R × T / P

V = 3.00 mol × 0.0821 atm.L/mol.K × 260 K / 0.800 atm

V = 80.0 L

Answer 2

Answer:

79.95L

Explanation:

Step 1:

Data obtained from the question. This include the information:

Temperature (T) = - 13°C

Pressure (P) = 0.800 atm

Number of mole (n) = 3.00 moles

Volume (V) =?

Step 2:

Conversion of celsius temperature to Kelvin temperature. This is illustrated below:

K = °C + 273

T = - 13°C = - 13°C + 273 = 260K

Step 3:

Determination of the volume of the gas. This is illustrated below:

Applying the ideal gas equation PV = nRT, the volume (V) of the gas can be obtained as follow:

The gas constant (R) = 0.082atm.L/Kmol

P = 0.8atm

n = 3 moles

T = 260K

PV = nRT

0.8 x V = 3 x 0.082 x 260

Divide both side by 0.8

V = (3 x 0.082 x 260) /0.8

V = 79.95L

Therefore, the volume of the gas in the balloon is 79.95L