A mixture of carbon dioxide and hydrogen gases, at a total pressure of 958 mmHg,

Question

A mixture of carbon dioxide and hydrogen gases, at a total pressure of 958 mmHg, contains 11.0 grams of carbon dioxide and 0.145 grams of hydrogen. What is this the partial pressure of each gas?
Pressure CO2= ? mm Hg Pressure H2= ? mm Hg A mixture of carbon dioxide and hydrogen gases, at a total pressure of 958 mmHg, contains 11.0 grams of carbon dioxide and 0.145 grams of hydrogen. What is this the partial pressure of each gas?
Pressure CO2= ? mm Hg Pressure H2= ? mm Hg
Pressure CO2= ? mm Hg Pressure H2= ? mm Hg

Explanation / Answer

we know that

moles = mass / molar mass

so

moles of C02 = 11 /44

moles of C02 = 0.25

now

moles of H2 = 0.145 / 2 = 0.0725

now

total moles = moles of C02 + moles of H2

total moles = 0.25 + 0.0725

total moles = 0.3225

now

mole fraction of C02 = moles of C02 / total moles

mole fraction of C02 = 0.25 / 0.3225

mole fraction of C02 = 0.775

now

mole fraction of C02 + mole fraction of H2 = 1

so

mole fraction of H2 = 1- 0.775

mole fraction of H2 = 0.225

now

we know that

pressure of C02 = mole fraction x total pressure

= 0.775 x 958

= 742.45

so

pressure of C02 = 742.45 mm Hg

now

pressure of H2 = total pressure - pressure of C02

pressure of H2 = 958 - 742.45

pressure of H2 = 215.55

so

pressure of H2 = 215.55 mm Hg

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