Question
How do I go about solving this reaction?
H2SO4 + NaCO3 = NaSO4 +CO2 + H2O
If 150.0g of sulfuric acid is spilled, what is the minimum number of sodium carbonate that have to be added to complete the reaction?
H2SO4 + NaCO3 = NaSO4 +CO2 + H2O
If 150.0g of sulfuric acid is spilled, what is the minimum number of sodium carbonate that have to be added to complete the reaction?
Answers
First, we need to correct the equation.
H2SO4 + Na2CO3 ==> Na2SO4 + CO2 + H2O
mols H2SO4 = 150 g/98 (molar mass H2SO4) = 1.53 moles H2SO4.
Using the coefficients in the balanced equation, convert moles H2SO4 to moles Na2CO3.
1.53 moles H2SO4 x (1 mole Na2CO3/1 mol H2SO4) = 1.53 x 1 = 1.53 moles Na2CO3.
Now convert moles Na2CO3 to grams. g = moles x molar mass.
H2SO4 + Na2CO3 ==> Na2SO4 + CO2 + H2O
mols H2SO4 = 150 g/98 (molar mass H2SO4) = 1.53 moles H2SO4.
Using the coefficients in the balanced equation, convert moles H2SO4 to moles Na2CO3.
1.53 moles H2SO4 x (1 mole Na2CO3/1 mol H2SO4) = 1.53 x 1 = 1.53 moles Na2CO3.
Now convert moles Na2CO3 to grams. g = moles x molar mass.