Question

A balloon is filled to a volume of 24.9L at a temperature of 27.1ºC. If the pressure in the balloon is measured to be 2.20 atm, how many moles of gas are contained inside the balloon?

Answer 1

Answer:

$n=2.20mol$

Explanation:

Hello,

In this case, we consider the ideal gas equation:

$PV=nRT$

For us to compute the required moles of the gas under the given conditions:

$n=\frac{PV}{RT}=\frac{2.20atm*24.9L}{0.082\frac{atm*L}{mol*K}*300.25K}\\ \\n=2.20mol$

Best regards.

Answer 2

Answer:

Inside the balloon we have 2.22 moles of gas

Explanation:

Step 1: Data given

A balloon is filled to a volume of 24.9L

Temperature is 27.1 °C = 300.25 K

The pressure of the balloon is measured to be 2.20 atm

Step 2: Calculate the number of moles

p*V = n*R*T

⇒with p = the pressure of the balloon = 2.20 atm

⇒with V = the volume of the balloon = 24.9 L

⇒with n = the number of moles of gas = TO BE DETERMINED

⇒with R = the gas constant = 0.08206 L* atm/mol*K

⇒with T = the temperature = 300.25 K

n= (p*V) / (R*T)

n = (2.20 * 24.9) / (0.08206 * 300.25)

n = 2.22 moles

Inside the balloon we have 2.22 moles of gas