TS EAMCET · Chemistry · States of Matter
Equal amounts of two gases of molecular weights 4 and 40 are mixed. The pressure of the mixture is 1.1 atm. What will be the partial pressure of the lighter gas in the mixture?
- A \(0.25 \mathrm{~atm}\)
- B \(0.5 \mathrm{~atm}\)
- C \(0.8 \mathrm{~atm}\)
- D \(1 \mathrm{~atm}\)
Answer & Solution
Correct Answer
(D) \(1 \mathrm{~atm}\)
Step-by-step Solution
Detailed explanation
Given, pressure of mixture \(\left(p_0\right)=1.1 \mathrm{~atm}\) Molecular weight of two gases \(=4\) and 40 . \(\therefore\) Number of moles of lighter gas \(=m / 4\) where, \(m=\) mass of gases and, number of moles of heavier gas \(=\frac{m}{40}\) Thus, total number of moles…
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