Problem: The hydrogen gas formed in a chemical reaction is collected over water at 30.0 °C at a total pressure of 732 mm Hg.a. What is the partial pressure of the hydrogen gas collected in this way?b. If the total volume of gas collected is 722 mL, what mass of hydrogen gas is collected? 

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FREE Expert Solution

We’re being asked to find the partial pressure and the mass of the hydrogen gas produced from a chemical reaction that is collected over water.

Hydrogen gas is the natural form of hydrogen and it is a diatomic molecule.

Hydrogen gas → H2(g)


(a) Partial Pressure of hydrogen gas

Given:            Total Pressure (Ptotal) = 732 mmHg


Dalton’s Law states that the total pressure inside a container is obtained by adding all the partial pressures of each non-reacting gas

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Problem Details

The hydrogen gas formed in a chemical reaction is collected over water at 30.0 °C at a total pressure of 732 mm Hg.

a. What is the partial pressure of the hydrogen gas collected in this way?

b. If the total volume of gas collected is 722 mL, what mass of hydrogen gas is collected?

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Based on our data, we think this problem is relevant for Professor Dabney's class at UTC.