Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc. Zn ( s ) + 2HC1 ( a q ) → ZnCl 2 ( a q ) + H 2 ( g ) Typically, the hydrogen gas is bubbled through water for collection and becomes saturated with water vapor. Suppose 240. mL of hydrogen gas is collected at 30°C and has a total pressure of 1.032 atm by this process. What is the partial pressure of hydrogen gas in the sample? How many grams of zinc must have reacted to produce this quantity of hydrogen? (The vapor pressure of water is 32 torr at 30°C.)

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Interpretation Introduction Interpretation: The partial pressures hydrogen gas in the given sample and number of grams of zinc is reacted in sample are needed to be determined. Concept introduction: Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone. Total pressure of a flask containing mixture of gases is the sum of individual partial pressures of constituted gases. Number of moles of a substance, According to ideal gas equation, Number of moles = Pressure × Volume R × Temperature Number of grams of a substance from its number of moles is, Number of moles × Molecular mass in grams = Number of grams Explanation Explanation To find: the Partial pressure of H 2 in the sample The Partial pressure of H 2 in the sample is 0.990 atm . The total pressure of the sample is given as 1 .032 atm . The partial pressure of water in the sample is given as 32 torr = 32 torr × 1 atm 760 torr = 0 .042 atm The total pressure of sample contains partial pressure of hydrogen and water. Therefore, The Partial pressure of H 2 in the sample is, 1 .032 atm - 0 .042 atm = 0 .990 atm To find: the number of moles of hydrogen gas in the sample. The number of moles of hydrogen gas is 9 .56 × 10 -3 mol . The Partial pressure of H 2 in the sample is calculated as 0.990 atm . The volume of hydrogen gas is given as 240 mL = 0 .240 L . The temperature of hydrogen gas is given as 30 o C = 30 3 K . The equation for finding number of moles of a substance, According to ideal gas equation, Number of moles = Pressure × Volume R × Temperature Therefore, The number of moles of hydrogen gas is, Number of moles = 0

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Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

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Interpretation Introduction

Interpretation: The partial pressures hydrogen gas in the given sample and number of grams of zinc is reacted in sample are needed to be determined.

Concept introduction:

Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.
Total pressure of a flask containing mixture of gases is the sum of individual partial pressures of constituted gases.

Number of moles of a substance, According to ideal gas equation,

Number of moles = Pressure × VolumeR × Temperature

Number of grams of a substance from its number of moles is,

Number of moles × Molecular mass in grams = Number of grams

Explanation of Solution

Explanation

To find: the Partial pressure of H2 in the sample

The Partial pressure of H2 in the sample is 0.990 atm .

The total pressure of the sample is given as 1.032 atm .

The partial pressure of water in the sample is given as 32 torr = 32 torr × 1 atm760 torr = 0.042 atm

The total pressure of sample contains partial pressure of hydrogen and water.

Therefore,

The Partial pressure of H2 in the sample is,

1.032 atm - 0.042 atm = 0.990 atm

To find: the number of moles of hydrogen gas in the sample.

The number of moles of hydrogen gas is 9.56 × 10-3 mol .

The Partial pressure of H2 in the sample is calculated as 0.990 atm .

The volume of hydrogen gas is given as 240 mL = 0.240 L .

The temperature of hydrogen gas is given as 30oC = 303 K .

The equation for finding number of moles of a substance, According to ideal gas equation,

Number of moles = Pressure × VolumeR × Temperature

Therefore,

The number of moles of hydrogen gas is,

Number of moles = 0

Chemistry: An Atoms First Approach

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