given 2C6H6+15O2->12CO2+6H2O

1. Starting with a confined volume of 4.80L and O2 with a partial pressure of 223.1 torr at 25 degrees C. C6H6 is in excess. The reaction is allowed to proceed to completion. The container is returned to 25C. Both liquid water and benzene are now present. The vapor pressure for benzene is 96.0 torr at 25C and vapor pressure of water at 25C is 24.0 torr. Calculate the total pressure. (you first need to calculate the CO2 pressure, which is its partial pressure)

Use PV = nRT and solve for n = mols O2.

Convert mols O2 to mols CO2 and mols H2O
Use PV = nRT and convert mols CO2 to pressure. I would then convert pCO2 in atm to torr.
Ptotal = pCO2 + pH2O + pC6H6.
Post your work if you get stuck.

To calculate the total pressure, you first need to determine the partial pressure of CO2. The balanced chemical equation shows that for every 2 moles of C6H6, 12 moles of CO2 are produced. Since C6H6 is in excess, we can assume that all 2 moles of C6H6 are used in the reaction, resulting in the production of 12 moles of CO2.

Given:
Partial pressure of O2 (PO2) = 223.1 torr
Vapor pressure of benzene (PBz) = 96.0 torr
Vapor pressure of water (PH2O) = 24.0 torr

The total pressure inside the container will be the sum of the partial pressures of the individual gases. To calculate the partial pressure of CO2 (PCO2), use Dalton's Law of Partial Pressures:

PCO2 = Ptotal - PO2 - PBz - PH2O

Since we are given the partial pressure of O2, we need to calculate the total pressure first.

To calculate the total pressure, we need to consider the ideal gas law:

PV = nRT

Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature (in Kelvin)

Since we are given the volume (4.80 L) and temperature (25 degrees C), we can convert the temperature to Kelvin:

T(K) = T(C) + 273.15 = 25 + 273.15 = 298.15 K

Now that we have the volume and temperature, we can solve for the number of moles of O2:

PV = nRT
n = (PV) / (RT)

n(O2) = ((223.1 torr) / (760 torr/atm)) * (4.8 L) / (0.0821 L*atm/mol*K) * (298.15 K)

Calculate the value and you will find the number of moles of O2.

Next, you know from the balanced chemical equation that for every 15 moles of O2, 12 moles of CO2 are produced. So divide the number of moles of O2 by 15 and multiply by 12 to find the number of moles of CO2.

Now that you have the number of moles of CO2, you can calculate its partial pressure (PCO2):

PCO2 = (nCO2 / ntotal) * Ptotal

Where:
nCO2 = Number of moles of CO2
ntotal = Total number of moles of all gases present (sum of moles of O2, CO2, benzene, and water)
Ptotal = Total pressure

Substitute the values into the equation and solve for PCO2.

Finally, calculate the total pressure by summing up all the partial pressures:

Ptotal = PO2 + PBz + PH2O + PCO2

Substitute the known values and the calculated value of PCO2 into the equation to find the total pressure.