Type the correct answer in the box. express your answer to three significant figures. a balloon is filled with 0.250 mole of air at 35°c. if the volume of the balloon is 6.23 liters, what is the absolute pressure of the air in the balloon? the absolute pressure of the air in the balloon is kilopascals.

∴ The absolute pressure of the air in the balloon in kPa = 102.69 kPa.

Explanation:

PV = nRT, where,

P is the pressure of the gas (atm),

V is the volume of the gas in L (V of air = 6.23 L),

n is the no. of moles of gas (n of air = 0.25 mole),

R is the general gas constant (R = 0.082 L.atm/mol.K),

T is the temperature of gas in K (T = 35 °C + 273 = 308 K).

∴ P = nRT / V = (0.25 mole)(0.082 L.atm/mol.K)(308 K) / (6.23 L) = 1.0135 atm.

1.0 atm → 101.325 kPa,

1.0135 atm → ??? kPa.

∴ The absolute pressure of the air in the balloon in kPa = (101.325 kPa)(1.0135 atm) / (1.0 atm) = 102.69 kPa.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.