Watch the following video on solving problems with Dalton's law. Then use what you learned to work to solve the following practice problems.

1. A mixture of neon and argon gases exerts a total pressure of 2.39 atm. The partial pressure of the neon alone is 1.84 atm, what is the partial pressure of the argon?
   
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   P_total = P1 + P2 + P3 + ...
   2.39atm = 1.84atm + P_argon
   P_argon = 2.39atm – 1.84atm
   P_argon = 0.55atm
2. A container that contains 20% oxygen, 30% hydrogen, and 50% nitrogen has a total pressure of 500kPa. What is the partial pressure of the hydrogen gas?
   
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   In a fixed volume the total pressure equals the sum of the partial pressures, so
   500kPa = (0.2_oxygen × 500kPa) + (0.3_hydrogen × 500kPa) + (0.5_nitrogen × 500kPa)
3. A mixture of oxygen, hydrogen, and nitrogen gases exerts a total pressure of 278 kPa. If the partial pressures of the oxygen and the hydrogen are 112 kPa and 101 kPa respectively, what would be the partial pressure exerted by the nitrogen?
   
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   P_{total = P1 + P2 + P3 + ...}
   278kPa = 112kPa + 101 kPa + P_nitrogen
   P_nitrogen = 278kPa – 112kPa – 101 kPa
4. A container has a mixture of 3 gases at a total pressure of 786 mmHg. The mixture contains 27% Gas A and 53% Gas B. What is the partial pressure due to the third gas?
   
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   The partial pressures due to Gas A and Gas B represent 80% of the total pressure (27% Gas A + 53% Gas B), so the partial pressure due to the third gas would equal 20% of the total pressure.
   786mmHg × 20% = 157.2mmHg