How many liters of CO2 would be collected over water from the bomcustion of 35g of cyclohexane, if the gas is collected at a barometric pressure of 765 torr and a temperature of 303 K?
To determine the number of liters of CO2 collected over water, we need to use the ideal gas law, which states:
PV = nRT
Where:
P is the pressure of the gas (in atmospheres)
V is the volume of the gas (in liters)
n is the number of moles of the gas
R is the ideal gas constant (0.0821 L•atm/mol•K)
T is the temperature of the gas (in Kelvin)
First, we need to convert the barometric pressure from torr to atmospheres.
1 atm = 760 torr
So, the pressure of 765 torr is approximately:
765 torr / 760 torr/atm = 1.0079 atm
Now, let's calculate the number of moles of CO2 using the given mass of cyclohexane.
1. Determine the molar mass of cyclohexane (C12H22)
Carbon (C) has a molar mass of 12.01 g/mol
Hydrogen (H) has a molar mass of 1.01 g/mol
Molar Mass of Cyclohexane = (12.01 g/mol) × 12 + (1.01 g/mol) × 22
2. Calculate the moles of cyclohexane using the given mass:
Moles of Cyclohexane = (35 g) / (Molar Mass of Cyclohexane)
3. Using the balanced equation for cyclohexane combustion, determine the stoichiometry between cyclohexane and CO2. Based on the balanced equation, one mole of cyclohexane produces 6 moles of CO2.
Moles of CO2 = (Moles of Cyclohexane) × 6
Now, we have the number of moles of CO2. We can rearrange the ideal gas law equation to solve for the volume of the gas:
V = (nRT) / P
Substituting the values:
V = [(Moles of CO2) × (0.0821 L•atm/mol•K) × (303 K)] / (1.0079 atm)
Finally, we can calculate the volume (V) of CO2 gas in liters.