If 2.5 grams of citric acid (H3C6H5O7) reacts, how many moles of carbon dioxide will be generated?
To determine the number of moles of carbon dioxide (CO2) generated when 2.5 grams of citric acid (H3C6H5O7) reacts, we need to follow these steps:
Step 1: Determine the molar mass of citric acid (H3C6H5O7).
The molar mass is calculated by adding up the atomic masses of all the atoms in the compound.
Molar mass of H: 1.01 g/mol
Molar mass of C: 12.01 g/mol
Molar mass of O: 16.00 g/mol
(3 * 1.01 g/mol) + (6 * 12.01 g/mol) + (7 * 16.00 g/mol) = 192.13 g/mol
The molar mass of citric acid is 192.13 g/mol.
Step 2: Convert the given mass of citric acid to moles.
To do this, we will use the formula: moles = mass / molar mass.
moles = 2.5 g / 192.13 g/mol = 0.013 moles
Step 3: Determine the mole ratio between citric acid and carbon dioxide.
The balanced chemical equation for the reaction will help us determine the mole ratio between citric acid and carbon dioxide. However, since the equation is not provided, we cannot determine the exact mole ratio.
For example, if the balanced equation is:
1 mole of citric acid (H3C6H5O7) + 3 moles of carbon dioxide (CO2) = 1 mole of citrate + 3 moles of water.
In this case, the mole ratio between citric acid and carbon dioxide is 1:3.
Step 4: Calculate the moles of carbon dioxide produced.
Using the mole ratio from step 3, we can calculate the moles of carbon dioxide produced.
moles of carbon dioxide = 0.013 moles (citric acid) * 3 moles (CO2) / 1 mole (citric acid)
moles of carbon dioxide = 0.039 moles
Therefore, if 2.5 grams of citric acid reacts, approximately 0.039 moles of carbon dioxide will be generated.