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?

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

explanation:

i think option no d is the correct answer

the maximum mass of nh3 is nh3 in grams