What is the partial pressure of hydrogen gas in a mixture that contains 6.00 grams of hydrogen gas and 1.80 mol carbon dioxide with a total pressure of 12.0 atm?

The partial pressure of hydrogen is equal to 7.5 atm.

Given the following data:

Scientific data:

To determine the partial pressure of hydrogen:

First of all, we would calculate the number of moles of hydrogen:

Number of moles = 3 moles

Next, we would determine the partial pressure of hydrogen:

Substituting the values, we have:

For hydrogen:

Partial pressure of hydrogen = 7.5 atm.

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P(H₂ ) =  7.5 atm

Explanation:

Given data:

Mass of hydrogen = 6.00 g

Number of moles of CO₂ = 1.80 mol

Total pressure = 12.0 atm

Partial pressure of H₂ = ?

Solution:

Number of moles of H₂:

Number of moles = mass/molar mass

Number of moles = 6.00 g/ 2 g/mol

Number of moles = 3 mol

Partial pressure of gases:

Total number of moles present = 1.80 mol + 3 mol = 4.80 mol

P(H₂ ) = [ 3 mol/ 4.80 mol] × 12.0 atm

P(H₂ ) = 0.625× 12.0 atm

P(H₂ ) =  7.5 atm

P(CO₂) = [1.80 mol/4.80 mol] × 12.0 atm

P(CO₂) = 0.375 × 12.0 atm

P(CO₂) = 4.5 atm

because u need two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei to form isotopes.

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