An experiment being conducted, the pressure is 0.9 atm and the temperature is 18 ° C. One of the steps of
experience requires the combustion of 500 ml of ethanol (d = 0.78 g / ml). Whereas the burning this amount of ethanol does not significantly alter the enviroments conditions, but releases carbon dioxide. Calculate the volume of CO2 generated (in L) and the CO2 concentration in mol / L
C2H5OH + 3O2 ==> 2CO2 + 3H2O
Determine mass ethanol from density.
mass = volume x density
mass = approx 400 but you need a more accurate answer than that.
mols ethanol = grams/molar mass = about 9 mols. Again you need to confirm an accurate answer.
For every 1 mol ethanol burned you get 2 mols CO2 so mols CO2 produced = approx 18.
Use PV = nRT to calculate volume in L.
(CO2) = mols/L. Plug in your value for mols and L to solve for (CO2).
Post your work if you get stuck.
and molarity of CO2 ?
I did that above.
(CO2) is read as concentration of CO2 in mols/L = M
Thank you :)
To calculate the volume of CO2 generated (in L) and the CO2 concentration in mol/L, we need to follow a few steps.
Step 1: Determine the number of moles of ethanol burned.
To do this, we need to use the density of ethanol (d = 0.78 g/ml) and the given volume (500 ml).
Mass of ethanol = Volume of ethanol × Density
Mass of ethanol = 500 ml × 0.78 g/ml
Step 2: Convert the mass of ethanol to moles.
To convert the mass of ethanol to moles, we need to know the molar mass of ethanol.
The molecular formula of ethanol is C2H5OH.
The atomic masses are:
C = 12.01 g/mol
H = 1.01 g/mol
O = 16.00 g/mol
Molar mass of ethanol = (2 × C) + (6 × H) + O
Molar mass of ethanol = (2 × 12.01 g/mol) + (6 × 1.01 g/mol) +16.00 g/mol
Now, we can calculate the moles of ethanol burned using the molar mass obtained and the mass of ethanol burned.
Moles of ethanol = Mass of ethanol / Molar mass of ethanol
Step 3: Calculate the volume of CO2 generated.
Since ethanol undergoes complete combustion, the carbon in ethanol is converted to CO2. The balanced equation for the combustion of ethanol is:
C2H5OH + 3O2 -> 2CO2 + 3H2O
According to the equation, 1 mole of ethanol produces 2 moles of CO2.
Volume of CO2 = (Moles of ethanol) × (2 moles of CO2 / 1 mole of ethanol)
Step 4: Convert the volume of CO2 to liters.
From the previous step, we have the volume of CO2 in moles. To obtain the volume in liters, we need to use the ideal gas law, which states:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin.
We need to convert the temperature from Celsius to Kelvin:
T (°C) = T (K) - 273.15
T (K) = 18 °C + 273.15
Now, we can calculate the volume of CO2 in liters using the ideal gas law:
Volume (L) = (Moles of CO2) × (0.0821 L·atm/(mol·K)) × (Temperature (K) / Pressure (atm))
Step 5: Calculate the CO2 concentration in mol/L.
The CO2 concentration in mol/L can be calculated by dividing the moles of CO2 by the volume (in liters) of the container.
CO2 concentration (mol/L) = Moles of CO2 / Volume of the container (L)
By following these steps, you can calculate the volume of CO2 generated (in L) and the CO2 concentration in mol/L for the given experiment.