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

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

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

explanation: