A student carries out a reaction in which 150.1 mL of hydrogen gas is generated and collected over water. The hydrogen gas is produced in a reaction between elemental zinc and an aqueous solution of hydrochloric acid. The total pressure of gases generated and collected in this reaction is 753.7 mmHg at a temperature of 30.0C. What mass (g) of hydrogen gas was collected in this reaction? (Vapor pressure of water at 30.0C = 31.86 mmHg)

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A common way to make hydrogen gas in the laboratory is to place a metal such as zinc in hydrochloric acid (see the figure). The hydrochloric acid reacts with the metal to produce hydrogen gas, which is then collected over water. Suppose a student carries out this reaction and collects a total of 140.2 mL of gas at a pressure of 749 mmHg and a temperature of 25∘C. What mass of hydrogen gas (in mg) does the student collect? (The vapor pressure of water is 23.78 mmHg at 25∘C.)

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A common way to make hydrogen gas in the laboratory is to place a metal such as zinc in hydrochloric acid (see the figure). The hydrochloric acid reacts with the metal to produce hydrogen gas, which is then collected over water. Suppose a student carries out this reaction and collects a total of 144.8 mL of gas at a pressure of 749 mmHg and a temperature of 25âC. What mass of hydrogen gas (in milligrams) does the student collect? (The vapor pressure of water is 23.78 mmHg at 25âC.)