Respuesta :
Answer:
There will react 0.400 moles of oxygen.
Explanation:
Step 1: Data given
Volume of the closed flask = 200.00 mL = 0.2 L
Number of moles of CO = 2.000 mol
Number of moles of O2 = 2.000 mol
Temperature = 300.0 K
Pressure decreases with 10%
Step 2: The balanced equation
2CO(g)+O2(g)⟶2CO2(g)
Step 3: Calculate the initial pressure of the flask before the reaction
P = nRT/V
⇒ with n = the number of moles (2.000 moles CO + 2.000 moles O2 = 4.000 moles)
⇒ R is gas constant (0.08206 atm*L/mol*K)
⇒T = the temperature = 300.0K
⇒ V = the volume = 200.0 mL = 0.2 L
P = (4 * 0.08206*300)/0.2
P = 492.36 atm
Step 4: When the pressure is 10 % decreased:
The final pressure = 492.36 - 49.236 = 443.124 atm
Step 5: Calculate the number of moles
n = PV/RT
⇒ with n = the number of moles
⇒ with P = the pressure = 443.124 atm
⇒ V = the volume = 200.0 mL = 0.2 L
⇒ R is gas constant (0.08206 atm*L/mol*K)
⇒T = the temperature = 300.0K
n =(443.124*0.2)/(0.08206*300)
n = 3.6 moles = total number of moles
Step 6: Calculate number of moles
For the reaction :2CO(g) + O₂(g) ⟶ 2CO₂(g)
For each mole of O2 we have 2 moles of CO, to produce 2 moles of CO2
Moles CO = (2 -2X) moles
Moles O2 = (2-X) moles
Moles CO2 = 2X
The total number of moles (4 -X)= 3.6 moles
Where X are moles that react
X = 0.400 moles
There will react 0.400 moles of oxygen.
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.
