Question:
The density of a gas is \( 1.964 \text{ g/dm}^{3} \) at \( 273 \text{ K} \) and \( 76 \text{ cm Hg} \). The gas is:
The density of a gas is \( 1.964 \text{ g/dm}^{3} \) at \( 273 \text{ K} \) and \( 76 \text{ cm Hg} \). The gas is:
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At STP, Molar Mass = Density $\times$ 22.4.
Updated On: Apr 8, 2026
- $CH_{4}$
- $C_{2}H_{6}$
- $CO_{2}$
- $Xe$
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The Correct Option is C
Solution and Explanation
Step 1: Concept
Use the ideal gas equation: $PV = nRT = \frac{w}{M}RT$, which gives $M = \frac{dRT}{P}$.
Step 2: Analysis
$d = 1.964 g/L$, $R = 0.0821 L\cdot atm/K\cdot mol$, $T = 273 K$, $P = 1 atm$.
$M = \frac{1.964 \times 0.0821 \times 273}{1} \approx 44$.
Step 3: Conclusion
The molar mass of $CO_{2}$ is $44 g/mol$.
Final Answer: (C)
Use the ideal gas equation: $PV = nRT = \frac{w}{M}RT$, which gives $M = \frac{dRT}{P}$.
Step 2: Analysis
$d = 1.964 g/L$, $R = 0.0821 L\cdot atm/K\cdot mol$, $T = 273 K$, $P = 1 atm$.
$M = \frac{1.964 \times 0.0821 \times 273}{1} \approx 44$.
Step 3: Conclusion
The molar mass of $CO_{2}$ is $44 g/mol$.
Final Answer: (C)
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