How many liters of Carbon Dioxide are formed by burning 6011.0 grams of C3H7OH with excess of oxygen gas and is carried out at 20.00 degrees Celsius, and 1.150 atm of pressure.
I know this needs PV=nRT but the burning and excess part is throwing me off. Please help me learn how to do this!
2C3H7OH + 9O2 ==> 6CO2 + 8H2O
mols C3H7OH = grams/molar mass = ?
Using the coefficients in the blanced equation, convert mols C3H7OH to mols CO2.
Now convert mols CO2 to L by
PV = nRT using the conditions of the problem.
To calculate the number of liters of carbon dioxide formed by burning ethanol (C3H7OH), we need to use the ideal gas law equation, 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.
Step 1: Convert grams to moles
To determine the number of moles of ethanol (C3H7OH) being burned, divide the given mass of ethanol (6011.0 grams) by its molar mass. The molar mass of C3H7OH can be calculated by adding up the atomic masses of its constituent elements:
Molar mass of C = 12.01 grams/mol
Molar mass of H = 1.01 grams/mol
Molar mass of O = 16.00 grams/mol
Molar mass of C3H7OH = (3 × 12.01) + (8 × 1.01) + 16.00 = 60.11 grams/mol
Number of moles of C3H7OH = mass of C3H7OH / molar mass of C3H7OH
= 6011.0 grams / 60.11 grams/mol
≈ 100 moles
Step 2: Balance the combustion equation and determine the stoichiometry
The combustion of ethanol can be represented by the balanced chemical equation:
C3H7OH + O2 → CO2 + H2O
From the balanced equation, we can see that for every mole of C3H7OH burned, one mole of CO2 is formed. Therefore, the number of moles of CO2 formed in this reaction is also 100.
Step 3: Convert moles to liters
Now, we need to convert the number of moles of CO2 to liters using the ideal gas law.
First, convert the temperature from Celsius to Kelvin by adding 273.15:
T = 20.00 + 273.15 = 293.15 K
Next, determine the pressure in atmospheres. Since the problem states that the pressure is 1.150 atm, we can directly use this value.
Finally, substitute the values into the ideal gas law equation:
PV = nRT
V = (nRT) / P
= (100 mol) × (0.0821 L·atm/mol·K) × (293.15 K) / (1.150 atm)
≈ 2200 L
Therefore, approximately 2200 liters of CO2 are formed by burning 6011.0 grams of C3H7OH.