Question:
A container consisting mixture of \(28 \mathrm{~g} \mathrm{~N}_2, 8 \mathrm{~g} \mathrm{He}\) and 40 g Ne at \(25^{\circ} \mathrm{C}\). If the total pressure exerted by the gaseous mixture is 20 bar , What is the partial pressure exerted by \(\mathrm{N}_2\) ?
A container consisting mixture of \(28 \mathrm{~g} \mathrm{~N}_2, 8 \mathrm{~g} \mathrm{He}\) and 40 g Ne at \(25^{\circ} \mathrm{C}\). If the total pressure exerted by the gaseous mixture is 20 bar , What is the partial pressure exerted by \(\mathrm{N}_2\) ?
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Find the mole fraction of nitrogen and multiply by the total pressure.
Updated On: Nov 13, 2026
- 2 bar
- 5 bar
- 4 bar
- 8 bar
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Verified By Collegedunia
The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept
Partial pressure \( =\) mole fraction \( \times \) total pressure.
Step 2: Moles
\( \text{N}_2=\dfrac{28}{28}=1 \), \( \text{He}=\dfrac{8}{4}=2 \), \( \text{Ne}=\dfrac{40}{20}=2 \)
Total \( =5 \text{ mol} \).
Step 3: Partial Pressure
\( p_{\text{N}_2}=\dfrac{1}{5}\times20=4 \text{ bar} \)
Step 4: Compare the options
This matches option (C).
Final Answer:
The partial pressure of nitrogen is 4 bar. \[ \boxed{\text{(C) }\text{4 bar}} \]
Partial pressure \( =\) mole fraction \( \times \) total pressure.
Step 2: Moles
\( \text{N}_2=\dfrac{28}{28}=1 \), \( \text{He}=\dfrac{8}{4}=2 \), \( \text{Ne}=\dfrac{40}{20}=2 \)
Total \( =5 \text{ mol} \).
Step 3: Partial Pressure
\( p_{\text{N}_2}=\dfrac{1}{5}\times20=4 \text{ bar} \)
Step 4: Compare the options
This matches option (C).
Final Answer:
The partial pressure of nitrogen is 4 bar. \[ \boxed{\text{(C) }\text{4 bar}} \]
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