Answer :
Answer:
0,400 moles of Oxygen
Explanation:
Using PV = nRT it is possible to obtain the initial pressure of the flask before the reaction thus:
P = nRT/V
Where:
n are moles (4,000 moles, 2,000 of CO and 2,000 moles of H₂O)
R is gas constant (0,082atmL/molK)
T is temperature (300,0K)
V is volume (0,2000L)
Replacing, P = 492,0 atm
If you want to decrease the pressure in 10,00%, the final pressure must be:
492,0atm - 49,2 atm = 442,8 atm
Solving under the same conditions with this pressure, moles must be:
n = PV/RT
n = 3,600 total moles
In the reaction:
2CO(g) + O₂(g) ⟶ 2CO₂(g)
The moles you will have are:
CO: 2,000 moles - 2X
O₂: 2,000 moles - X
CO₂: 2X
Where X are moles that react
Thus, total moles are:
4,000moles - X = 3,600 moles
X = 0,400 moles
That means that moles of oxygen that have to react are 0,400 moles of Oxygen
I hope it helps!
Answer: 0.4000 mol
Explanation:
In a closed flask with fixed volume, the number of moles of ideal gas is proportional to the pressure.
P∝n
To decrease the overall pressure by 10.00%, the number of moles should be decreased by 10.00% as well. Therefore, the number of moles must be decreased by
4.000 mol × 0.1000 = 0.4000 mol
Consider the equation for this reaction.
2CO(g)+O2(g)⟶2CO2(g)
In the balanced equation, 2 mol of carbon monoxide gas (CO) reacts with 1mol of oxygen gas to form 2 mol of carbon dioxide CO2. Notice that the change in the total number of moles is equal to the number of moles of oxygen that react. Therefore, if the total amount of gas decreases by 0.4000 mol, then 0.4000 mol of oxygen gas must react with carbon monoxide. In this case, 0.8000 mol of carbon monoxide is consumed and 0.8000 mol of carbon dioxide is produced.