In H2SO4 + 2NaOH = 2H2O + Na2SO4
How much of the excess reagent will remain after the reaction has been completed?
I know that NaOH is the limiting reactant
Depends on how much sulfuric acid was used.
How do i figure out how much of it was used?
To determine how much of the excess reagent (in this case, H2SO4) remains after the reaction has completed, you need to follow a few steps:
1. Determine the moles of the limiting reactant (NaOH) used in the reaction. This can be calculated using the stoichiometry of the balanced equation. In this case, there is a 1:2 molar ratio between NaOH and H2SO4. So for every 2 moles of NaOH used, 1 mole of H2SO4 is used.
2. Convert the moles of the limiting reactant (NaOH) to the moles of the excess reactant (H2SO4) using the stoichiometry mentioned above.
3. Compare the moles of the excess reactant (H2SO4) obtained in step 2 to the moles of the excess reactant initially present.
4. Calculate the remaining moles of the excess reactant (H2SO4) by subtracting the moles used in the reaction from the initial moles.
5. Finally, convert the moles of the remaining excess reactant (H2SO4) to grams (if required) using its molar mass.
By following these steps, you can determine the amount of excess reagent (H2SO4) that will remain after the reaction has completed.