Assuming the temperature of the system is 20 C the atmospheric pressure is 0.998 atm, and the total volume collected in the balloon is 0.28 L, calculate the number of moles of H2 collected in the ballot. This is the actual yield. Use the dalton's law of partial pressure to determine the partial pressure of H2 in the balloon. The vapor pressure of water is 20 Cis 17.5 mmHg

The number of moles of H₂ is 0.01135 moles

The partial pressure of H₂ in the balloon is 0.975 atm

Explanation:

From Dalton's law of partial pressure, we have;

Total pressure = Pressure of H₂ + Pressure of the water vapor

The vapor pressure of water at 20°C = 17.5 mmHg = 0.0230225 atm

For equilibrium, pressure of the balloon = Surrounding pressure = Atmospheric pressure

∴ Pressure of H₂ + Pressure of the water vapor = Atmospheric pressure

Partial pressure of H₂ in the balloon, P = 0.998 - 0.0230225 = 0.9749775 ≈ 0.975 atm

0.975 atm  = 98789.595 Pa

Volume of balloon, V = 0.28 L

n = PV/(RT)

Where:

R = Universal gas constant = 0.08205 L·atm/(mol·K)

T = Temperature = 20°C = 293.15 K

∴ n = 0.975 * 0.28/ (0.08205  * 293.15) =  0.01135 moles.

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