Respuesta :
Answer:
CO = zero
CO2 =1 bar
O2 = 2.02 bar
Explanation:
We are given
initial pressure of CO = 1bar
total pressure = 3.52 bar
so initial pressure of O2 = 3.52 - 1 = 2.52 bar
the reaction is
2CO + O2 → 2CO2
using the unitary method
2 moles of CO2 → 1 mole of O2
1 bar of CO → [tex]\frac{1}{2} * 1= 0.5 bar[/tex] (required)
but we have more oxygen present , that means CO is the limiting reagent
- Final pressure of CO will be zero as it is the limiting reagent so it will be consumed completely
- 1 bar of CO → [tex]\frac{2mol CO2}{2mol CO} * 1= 1 bar[/tex] of CO2
- 2.52 bar O2 (initially) - 0.5 bar (reacted) = 2.02bar O2
I. The final partial pressure of carbon monoxide (CO) is zero (0) bar.
II. The final partial pressure of molecular oxygen ([tex]O_2[/tex]) is 2.02 bar.
Given the following data:
- Initial volume = 50.0 Liters
- Initial temperature = 25.0°C
- Initial pressure of CO = 1.00 bar
- Total pressure = 3.52 bar.
- Heating temperature = 350.0°C
- Final temperature = 25.0°C
To compute the final partial pressure of each gas (in bar):
The balanced chemical reaction is written as:
[tex]2CO + O_2 ---> 2C0_2[/tex]
First of all, we would determine the initial pressure of oxygen.
[tex]Initial\;pressure\;of\;O_2 = Total\;pressure - Initial\;pressure\;of\;CO\\\\Initial\;pressure\;of\;O_2 = 3.52 - 1\\\\Initial\;pressure\;of\;O_2 = 2.52 \;bar[/tex]
By stoichiometry:
2 mole of CO = 1 mole of [tex]O_2[/tex]
1 bar of CO = X bar of [tex]O_2[/tex]
Cross-multiplying, we have:
[tex]X=\frac{1}{2} \;bar[/tex]
Since carbon monoxide (CO) is the limiting agent, it's final partial pressure would be equal to zero (0) bar because it reacted completely with the molecular oxygen.
For molecular oxygen:
[tex]Final\;partial\;pressure = 2.52 - 0.5[/tex]
Final partial pressure = 2.02 bar.
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