Question:
A container contains equal masses of \(\mathrm{H}_2, \mathrm{He}\), \(\mathrm{CO}_2\) and Ne at a certain temperature. Which of the following gas exerts maximum partial pressure?
A container contains equal masses of \(\mathrm{H}_2, \mathrm{He}\), \(\mathrm{CO}_2\) and Ne at a certain temperature. Which of the following gas exerts maximum partial pressure?
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Partial pressure is proportional to the number of moles, and for equal masses moles are inversely proportional to molar mass.
Updated On: Nov 13, 2026
- \(\mathrm{H}_{2}\)
- He
- \(\mathrm{CO}_{2}\)
- Ne
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Concept
By Dalton's law, partial pressure of a gas is \(p_i=x_iP_{\text{total}}\), so it is proportional to its number of moles.
Step 2: Moles for equal mass
For mass \(w\) of each gas, \(n=w/M\).
Molar masses: \(\text{H}_2=2\), He \(=4\), \(\text{CO}_2=44\), Ne \(=20\) g/mol.
Step 3: Compare
The gas with the smallest molar mass has the most moles.
\(\text{H}_2\) has the smallest molar mass, so it has the largest mole fraction and the highest partial pressure.
Final Answer:
Hydrogen exerts the maximum partial pressure. \[ \boxed{\text{(A) }\text{H}_{2}} \]
By Dalton's law, partial pressure of a gas is \(p_i=x_iP_{\text{total}}\), so it is proportional to its number of moles.
Step 2: Moles for equal mass
For mass \(w\) of each gas, \(n=w/M\).
Molar masses: \(\text{H}_2=2\), He \(=4\), \(\text{CO}_2=44\), Ne \(=20\) g/mol.
Step 3: Compare
The gas with the smallest molar mass has the most moles.
\(\text{H}_2\) has the smallest molar mass, so it has the largest mole fraction and the highest partial pressure.
Final Answer:
Hydrogen exerts the maximum partial pressure. \[ \boxed{\text{(A) }\text{H}_{2}} \]
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