A helium balloon can hold about 6.8 mol of the gas. Assuming the balloon is kept at room temperature (25°C) and had a maximum of 1.2L, what is the pressure inside teh balloon

P = 138.6 atm or 1.4x10²

Explanation:

You will need to use PV=nRT to solve for P, pressure

Where the R constant is 0.08206 L atm mol^-1 K^-1

V is 1.2 L

T is temperature in kelvin, 273.15+25 = 298.15

n is 6.8 mol

P*1.2=6.8*0.08206*298.15 - --> P*1.2=166.3700852 - --> P=166.3700852/1.2

P=138.6 atm

or 1.4x10²

138.47atm

Explanation:

Data obtained from the question include:

n (number of mole) = 6.8 mol

T (temperature) = 25°C = 25 + 273 = 298K

V (volume) = 1.2L

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

P (pressure) = ?

Using the ideal gas equation PV = nRT, we can confidently calculate the pressure inside the balloon as shown below:

PV = nRT

P = nRT/V

P = (6.8 x 0.082 x 298) / 1.2

P = 138.47atm

Therefore, the pressure inside the balloon is 138.47atm