Copper reacts with sulfuric acid according to the following equation: 2H3SO4 + Cu-> CuSO4 + 2H2O + SO2 How many grams of sulfur dioxide are created by this reaction if 14.2 g of copper reacts with 18 g of sulfuric acid?

Answer 1

You have a limiting regent problem here. Basically, you work two stoichiometry problems and take the one producing the smaller amount of product as the valid one.
1. Convert 14.2 g Cu to moles. moles = grams/molar mass
2. Convert 18 g H2SO4 to moles using the same process.
3. Using the coefficients in the balanced equation, convert moles Cu to moles of the product.
4. Same procedure, convert moles H2SO4 5o moles of the product.
5. It is likely that the answer from 3 and 4 will not agree. The correct answer, in limiting reagent problems. is ALWAYS the smaller one.
6. Convert mole SO2 from step 5 to grams. g = moles x molar mass.
Post your work if you get stuck.

Answer 2

I don't understand step 3?