Answer:
0.400 moles of Oxygen
Explanation:
By employing the equation PV = nRT, the initial pressure of the flask can be calculated prior to the reaction, which leads to:
P = nRT/V
Where:
n signifies moles (4,000 moles: 2,000 moles of CO and 2,000 moles of H₂O)
R represents the gas constant (0.082 atm·L/mol·K)
T is the temperature (300.0 K)
V denotes volume (0.2000 L)
Substituting values results in P = 492.0 atm
To achieve a pressure reduction of 10.00%, the resulting pressure should be:
492.0 atm - 49.2 atm = 442.8 atm
Calculating with the new pressure under the same conditions gives the moles as:
n = PV/RT
n = 3,600 total moles
In the reaction:
2CO(g) + O₂(g) ⟶ 2CO₂(g)
The resulting moles are:
CO: 2,000 moles - 2X
O₂: 2,000 moles - X
CO₂: 2X
Where X accounts for the moles that react
Consequently, the total moles are:
4,000 moles - X = 3,600 moles
X = 0.400 moles
This indicates that the amount of oxygen needed for the reaction is 0.400 moles of Oxygen
I hope this is useful!
