The hydrogen gas formed in a chemical reaction is collected over water at 30.0 degrees c at a total pressure of 732 mmhg what is the partial pressure of the hydrogen gas collected

The partial pressure of the hydrogen gas collected : 700.4974 mmHg

Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases

Can be formulated:

The partial pressure is the pressure of each gas in a mixture

The hydrogen gas is formed in a chemical reaction evaporate and mixed with water vapor

Hydrogen gas pressure and water-vapor pressure produce total pressure of the gas

So

At 30.0 o C the vapor pressure of water is 4.2 kPa. (a vapor pressure table is in the attached picture)

Because 1kPa = 7,50062 mmHg, then 4.2 kPa = 31,5026 mmHg

So the partial pressure of the Hydrogen gas is

732 mmHg (P total) = 31.5026 mmHg (P water vapor) + P Hydrogen gas

 P Hydrogen gas = 732 - 31.5026

 P Hydrogen gas = 700.4974 mmHg

The combined gas law

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Chlorine gas

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The following pairs of properties

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explanation:

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