Carbon monoxide reacts with oxygen to form carbon dioxide.?

Question

2CO + O2 -> 2CO2
In a 1.00 L flask, 2.4 atm of CO reacts with 4.5 atm of O2. Assuming that the temperature remains constant, what is the final pressure in the flask?

Answer 1

The answer is 5,7
p(CO)=2,4 atm
1 mol CO reacts with half amount of O2 so 2,4 atm CO with 1,2 atm O2.
What we have from this reaction is CO2, (equal the amount of starting CO) => 2,4 atm.
But we need to add the remaining oxigen too; we used up 1,2 atm from the starting 4,5 atm, so what's left is (4,5-1,2=>) 3,3 atm O2.
The total pressure is the pressure of the CO2 and the O2 = 2,4+3,3= 5,7 atm.

Answer 2

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RE:
Carbon monoxide reacts with oxygen to form carbon dioxide.?
2CO + O2 -> 2CO2
In a 1.00 L flask, 2.4 atm of CO reacts with 4.5 atm of O2. Assuming that the temperature remains constant, what is the final pressure in the flask?

Answer 3

2 moles of CO reacts with one mole of O2. So the 2.4 atm of CO will react with 1.2 atm of O2 giving 2.4 atm CO2
from the 4.5 atm of O2 4.5-1.2 =3.3atm are not used . So, the final pressure would be 1.2+3.3 =4.5 atm

Remark : When you have a reaction it is not the atm which react but a number of moles. Care to units !

Answer 4

Because pressure is directly proportional to moles (PV = nRT) and because V and T are not changing, you can treat pressure in the same way as you would treat moles in terms of stoichiometry. So, find the limiting reactant, find how much product you produce, etc., and then you can find the total pressure once the reaction has completed.

Answer 5

it would be carbon monoxide because you can not convert that into caebon dioxide

Answer 6

2.4*2=4.8
4.5 of O2

4.8+4.5=9.3 is the total pressure