Answer:
There will react 0.400 moles of oxygen.
Explanation:
<u>Step 1:</u> 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%
<u>Step 2</u>: The balanced equation
2CO(g)+O2(g)⟶2CO2(g)
<u>Step 3</u>: 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
<u>Step 4:</u> When the pressure is 10 % decreased:
The final pressure = 492.36 - 49.236 = 443.124 atm
<u>Step 5:</u> 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
<u>Step 6:</u> 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.
= 150 molecules O₂
