Given: 2CO(g) + O2(g) -> 2C02(g). When 10 mol of CO and 8.0 mol of O2 react in a closed 10L vessel.
a)how many moles of CO, O2, and CO2 are present at the end of the reaction?
b)What will be the total pressure in the flask at 0 degrees C?
Are you assuming that the reaction goes to completion? You don't have a Kp or Kc listed.
What's the limiting reagent? I believe that is CO.
............2CO + O2 ==> 2CO2
I...........10....8........0
C..........-10...-5.......10
E...........0.....3.......10
So you have 13 mols at the end of the reaction. PV = nRT should give you the pressure.
To determine the number of moles of CO, O2, and CO2 present at the end of the reaction, we need to use the stoichiometry of the balanced chemical equation.
a) The balanced chemical equation shows that 2 moles of CO react with 1 mole of O2 to produce 2 moles of CO2. Therefore, for every 2 moles of CO, we need 1 mole of O2.
Given that we have 10 moles of CO and 8.0 moles of O2, we determine which reactant is the limiting reactant. The limiting reactant is the reactant that will be completely consumed first, thereby determining the maximum amount of product formed.
Since we need 2 moles of CO for every 1 mole of O2, we can calculate the number of moles of CO that can react with 8.0 moles of O2:
10 mol CO × (1 mol O2 / 2 mol CO) = 5.0 mol O2
Since our reaction mixture only contains 8.0 moles of O2, it is the limiting reactant. Therefore, 5.0 moles of O2 will react completely, forming 10 moles of CO2.
Now, to determine the remaining moles of CO, we subtract the moles of CO that reacted from the initial moles of CO:
10 mol CO - (5.0 mol O2 × (2 mol CO / 1 mol O2)) = 10 mol CO - 10 mol CO = 0 mol CO
Therefore, all 10 moles of CO have reacted, and there are 0 moles of CO left.
To summarize:
- Moles of CO at the end of the reaction: 0 mol
- Moles of O2 at the end of the reaction: 3.0 mol (8.0 mol O2 - (5.0 mol O2 × (1 mol O2 / 2 mol CO)))
- Moles of CO2 at the end of the reaction: 10 mol
b) To determine the total pressure in the flask at 0 degrees C, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, we are given:
- The volume of the flask is 10 L.
- The temperature is 0 degrees C, which is equivalent to 273.15 K.
To calculate the total pressure, we need to determine the number of moles of each gas present and substitute them into the ideal gas law.
- Moles of O2: 3.0 mol (as calculated above)
- Moles of CO2: 10 mol (as calculated above)
Now, we can use the ideal gas law to find the total pressure:
P(total) × V = n(total) × R × T
P(total) × 10 L = (3.0 mol + 10 mol) × R × 273.15 K
Simplifying the equation:
P(total) = (13.0 mol × R × 273.15 K) / 10 L
Finally, we substitute the ideal gas constant value, R = 0.0821 L·atm/mol·K:
P(total) = (13.0 mol × 0.0821 L·atm/mol·K × 273.15 K) / 10 L
Calculating this expression will give you the value of the total pressure in the flask at 0 degrees C.