Answer:
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
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:
[tex]Number\;of\;moles = \frac{mass}{molar\;mass}\\\\Number\;of\;moles = \frac{6.00}{2}[/tex]
Number of moles = 3 moles
Next, we would determine the partial pressure of hydrogen:
[tex]Molefraction \;of \;a \;substance =\frac{No.\; of \; moles \;of \;substance}{Total \;no. \;of \; moles \;of \;substances}[/tex]
Substituting the values, we have:
[tex]Molefraction \;of \;a \;substance =\frac{3}{4.8} \\\\Molefraction \;of \;a \;substance =0.625[/tex]
For hydrogen:
[tex]Partial \;pressure = Molefraction \times Total\;pressure\\\\Partial \;pressure = 0.625 \times 12.0[/tex]
Partial pressure of hydrogen = 7.5 atm.
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