Alveolar air (a mixture of nitrogen, oxygen, and carbon dioxide) has a total pressure of 0.998 atm. If the partial pressure of o
1 answer:
Answer:
The partial pressure of carbon dioxide is 22.8 mmHg
Explanation:
Dalton's Law is a gas law that relates the partial pressures of the gases in a mixture. This law says that the pressure of a gas mixture is equal to the sum of the partial pressures of all the gases present.
In this case:
Ptotal=Pnitrogen + Poxygen + Pcarbondioxide
You know that:
- Ptotal= 0.998 atm
- Pnitrogen= 0.770 atm
- Poxygen= 0.198 atm
- Pcarbondioxide= ?
Replacing:
0.998 atm=0.770 atm + 0.198 atm + Pcarbondioxide
Solving:
Pcarbondioxide= 0.998 atm - 0.770 atm - 0.198 atm
Pcarbondioxide= 0.03 atm
Now you apply the following rule of three: if 1 atm equals 760 mmHg, 0.03 atm how many mmHg equals?
Pcarbondioxide= 22.8 mmHg
<u><em>The partial pressure of carbon dioxide is 22.8 mmHg</em></u>
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Answer:
Approximately .
Explanation:
Make use of the molar mass data () to calculate the number of moles of molecules in that
of
:
.
Make sure that the equation for this reaction is balanced.
Coefficient of in this equation:
.
Coefficient of in this equation:
.
In other words, for every two moles of that this reaction consumes, two moles of
would be produced.
Equivalently, for every mole of that this reaction consumes, one mole of
would be produced.
Hence the ratio: .
Apply this ratio to find the number of moles of that this reaction would have produced:
.