Final answer:
To find the amount of CO2 produced from 380.0 g of HNO3 reacting with Na2CO3, we calculate the moles of HNO3, then use the stoichiometry of the reaction to find the moles, and finally the mass of CO2 produced. A total of 132.69 grams of CO2 would be produced.
Step-by-step explanation:
To determine how many grams of carbon dioxide (CO2) will be produced from 380.0 g of HNO3 reacting with an excess of Na2CO3, we first need to write a balanced chemical equation for the reaction. However, there seems to be a mistake as HNO3 would react with Na2CO3 differently compared to the reaction provided in the reference information. The actual reaction should be:
2 HNO3 + Na2CO3 → 2 NaNO3 + CO2 + H2O
This balanced equation shows that 1 mole of Na2CO3 produces 1 mole of CO2. The molar mass of HNO3 is 63.01 g/mol. So, the moles of HNO3 are:
Moles of HNO3 = 380.0 g ÷ 63.01 g/mol = 6.03 mol
Since 2 moles of HNO3 produce 1 mole of CO2, 6.03 moles of HNO3 will yield 3.015 moles of CO2. The molar mass of CO2 is 44.01 g/mol.
Mass of CO2 = 3.015 mol × 44.01 g/mol = 132.69 g
Therefore, 132.69 grams of CO2 will be produced from the reaction of 380.0 g of HNO3 with an excess of Na2CO3.