Suppose you used an excess of sulfuric acid in all the flasks. How many moles of CO2 would be released in flask 7 if the molar mass of sodium carbonate is 105.99 g/mol?

I would need information on how much sodium carbonate is present in Flask 7, as well as the concentration of the sulfuric acid used. The amount of CO2 released depends on the amount of sodium carbonate that reacts with the sulfuric acid. The balanced chemical equation for the reaction between sodium carbonate (Na2CO3) and sulfuric acid (H2SO4) is:

Na2CO3 + H2SO4 → Na2SO4 + CO2 + H2O

From the balanced equation, we see that 1 mole of sodium carbonate reacts with 1 mole of sulfuric acid to produce 1 mole of CO2. To find out how many moles of CO2 would be released, we need to know the moles of sodium carbonate in Flask 7.

Suppose you have 'x' grams of sodium carbonate in Flask 7. The number of moles of sodium carbonate (n) would be calculated as:

n(sodium carbonate) = mass (sodium carbonate) / molar mass (sodium carbonate) n(sodium carbonate) = x grams / 105.99 g/mol

The number of moles of CO2 produced would be equal to the number of moles of sodium carbonate reacting, which is n(sodium carbonate), assuming there is excess sulfuric acid so that all sodium carbonate can react.