AP EAMCET · Chemistry · States of Matter
What is the density of one mole of \(\mathrm{He}\) (molar mass \(=4 \mathrm{~g}\) \(\left.\mathrm{mol}^{-1}\right)\) at \(300 \mathrm{~K}\) and a pressure of \(0.82 \mathrm{~atm} ?(\mathrm{R}=0.082 \mathrm{~L}\) \(\left.\operatorname{atm} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)\)
- A \(1.33 \times 10^{-2} \mathrm{~g} \mathrm{~mL}^{-1}\)
- B \(1.33 \times 10^{-2} \mathrm{~g} \mathrm{~L}^{-1}\)
- C \(1.33 \times 10^{-1} \mathrm{~g} \mathrm{~L}^{-1}\)
- D \(1.33 \times 10^{-1} \mathrm{~g} \mathrm{~mL}^{-1}\)
Answer & Solution
Correct Answer
(C) \(1.33 \times 10^{-1} \mathrm{~g} \mathrm{~L}^{-1}\)
Step-by-step Solution
Detailed explanation
From ideal gas equation, \(\mathrm{PV}=\mathrm{nRT}\) or, \(\mathrm{PM}=\mathrm{dRT}\) \([\mathrm{d}=\) density of gas and \(\mathrm{M}=\) molecular/atomic weight of the gas] \(\therefore \quad \mathrm{d}=\frac{\mathrm{PM}}{\mathrm{RT}}\)…
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