A gas mixture contains helium (He ), argon (Ar) , neon (Ne ), Xenon ( Xe), and krypton (Kr) gases. The total pressure of the gas mixture is 1252.5 mm Hg. The partial pressures of He, Ar , Ne, and Xe are 0.32, 0.21, 0.44, and 0.19 atm, respectively. What is the partial pressure exerted by Kr?

0.488atm = Pressure Kr

Explanation:

The total pressure in a mixture of gases could be defined as the sum of the partial pressures of a mixture. For the mixture of gases in the problem:

Total pressure = Pressure He + Pressure Ar + Pressure Ne + Pressure Xe + Pressure Kr

Converting the total pressure to atm:

1252.5mm Hg * (1atm / 760 mmHg) = 1.648 atm

Replacing:

1.648atm = 0.32atm + 0.21atm + 0.44atm + 0.19atm + Pressure Kr

8 carbon atoms forming single bonds with 18 hydrogen atoms; a triple bond exists between the third and fourth carbon atom from the right

explanation:

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