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.

102.8 kPa.

Explanation:

We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm (P = ? atm).

V is the volume of the gas in L (V = 4000 mL = 6.23 L).

n is the no. of moles of the gas in mol (n = 0.25 mol).

R is the general gas constant (R = 0.0821 L. atm/mol. K),

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

∴ P = nRT/V = (0.25 mol) (0.0821 L. atm/mol. K) (308 K) / (6.23 L) = 1.015 atm.

To convert to kPa:

multiply the pressure value by 101.325

∴ P = (1.0 atm) (101.325 kPa/1.0 atm) = 102.8 kPa.