Answer:
4.401 g
Step-by-step explanation:
To determine the amount of carbon dioxide formed from 6.20 grams of carbonic acid, we first need to know the molar mass of carbonic acid (H2CO3).
The molar mass of carbonic acid can be calculated as:
Molar mass of carbonic acid (H2CO3) = (2 * atomic mass of hydrogen) + atomic mass of carbon + (3 * atomic mass of oxygen)
Molar mass of carbonic acid (H2CO3) = (2 * 1.01 g/mol) + 12.01 g/mol + (3 * 16.00 g/mol)
= 2.02 g/mol + 12.01 g/mol + 48.00 g/mol
= 62.03 g/mol
Now, we can calculate the number of moles of carbonic acid:
Number of moles of carbonic acid = (mass of carbonic acid) / (molar mass of carbonic acid)
= 6.20 g / 62.03 g/mol
= 0.0999 mol (approximately 0.1 mol)
From the balanced equation of the reaction, we know that 1 mole of carbonic acid produces 1 mole of carbon dioxide (CO2).
Therefore, the number of moles of carbon dioxide formed from 0.1 mol of carbonic acid is also 0.1 mol.
Finally, we can calculate the mass of carbon dioxide formed:
Mass of carbon dioxide = (Number of moles of carbon dioxide) * (molar mass of carbon dioxide)
= 0.1 mol * 44.01 g/mol
= 4.401 g
Therefore, 6.20 grams of carbonic acid will form approximately 4.401 grams of carbon dioxide.