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?

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

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