If 2.5 grams of citric acid (H3C6H5O7) reacts, how many grams of carbon dioxide will be generated?
2H3C6H5O7 + 9O2 ==> 12CO2 + 8H2O
mols citric acid = grams/molar mass
Convert mols citric acid to mols CO2 using the coefficients in the balanced equation. That/s ?mols citric acid x (12 mols CO2/2 mol cit acid) = ?
Now convert mols CO2 to grams. g = mols x molar mass.BTW this is called the theoretical yield.
To determine how many grams of carbon dioxide (CO2) will be generated when 2.5 grams of citric acid (C6H8O7) reacts, we need to use the balanced chemical equation for the reaction between citric acid and the bicarbonate ion (HCO3-):
3 H3C6H5O7 + 3 HCO3- → 3 H2O + 3 CO2 + C6H5O7-2
In this equation, we can see that for every 3 moles of citric acid (H3C6H5O7) that react, 3 moles of CO2 (carbon dioxide) are produced.
To solve this problem, we can follow these steps:
Step 1: Calculate the molar mass of citric acid (C6H8O7). The molar mass of C6H8O7 can be calculated by summing the atomic masses of all the atoms in the formula:
C: 6 x 12.01 g/mol = 72.06 g/mol
H: 8 x 1.01 g/mol = 8.08 g/mol
O: 7 x 16.00 g/mol = 112.00 g/mol
Total molar mass of C6H8O7 = 72.06 g/mol + 8.08 g/mol + 112.00 g/mol = 192.14 g/mol
Step 2: Convert the given mass of citric acid (2.5 grams) to moles. To do this, divide the mass by the molar mass:
2.5 g ÷ 192.14 g/mol = 0.013 moles (approx.)
Step 3: Calculate the moles of CO2 produced. Using the balanced equation, we can see that for every 3 moles of citric acid, 3 moles of CO2 are produced. Therefore, the number of moles of CO2 is the same as the number of moles of citric acid, which is 0.013 moles (approx.).
Step 4: Convert moles of CO2 to grams. Since the molar mass of CO2 is 44.01 g/mol, we can multiply the moles of CO2 by the molar mass to find the mass:
0.013 moles x 44.01 g/mol ≈ 0.57 grams
Therefore, approximately 0.57 grams of carbon dioxide (CO2) will be generated when 2.5 grams of citric acid (H3C6H5O7) reacts.