A balloon is floating around outside your window. The temperature outside is 7 degrees C, and the air pressure is 0.800atm . Your neighbor, who released the balloon, tells you that he filled it with 4.20moles of gas. What is the volume of gas inside this balloon?

Relevance

Ideal Gas Law: PV=nRT (P=pressure in atm, V= volume in liters, n= number of moles, R= .0821 (it's a

constant), and T= temperature in Kelvin)

Lets convert the temperature in Celsius to Kelvin by adding 273: 7+273= 280 Kelvin

Plug in what you have: PV=nRT -----> (0.8 atm)(V) = (4.2 moles)(.0821)(280 Kelvin)

(0.8 atm)(V)= 96.55

V = 120.687

The Volume is 120.687 liters.

Source(s): Chem Honors & AP Chem :)
• Plug this into the equation PV=nRT <-- this is the ideal gas law and helps us figure out values given the relationships between pressure (P), Volume (V), moles (n), The ideal gas constant (R), and Temperature (T).

R-ideal gas constant 0.0821 (L * atm) / (K * mol)

You must use all the units that are included in the ideal gas constant, so you will need to do some stoichiometry to convert degrees C to Kelvin in this situation so:

7. degrees C + 273.15= 280.15 K

Now plug that in for T, Plug in 4.20 moles for n, plug in 0.0800 atm for P, and 0.0821 (L * atm) / (K * mol) for R. Then do some algebra to get V (Volume in Liters). To make it easier, you can re situate the Ideal gas law formula to equal V--> V=nRT/P. Make sure you have the right number of sig figs in your answer.

Source(s): I just learned this in my General Chemistry class actually.