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?
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.
To solve this reaction, you need to use stoichiometry, which involves calculating the amount of reactants and products based on their balanced mole ratios.
First, let's balance the equation:
H2SO4 + NaCO3 = NaSO4 + CO2 + H2O
The balanced equation shows that 1 mole of H2SO4 reacts with 1 mole of NaCO3 to produce 1 mole of NaSO4, 1 mole of CO2, and 1 mole of H2O.
To determine the minimum number of moles of NaCO3 needed to react with 150.0g of H2SO4, you need to follow these steps:
1. Calculate the number of moles of H2SO4:
Moles = Mass of substance (g) / Molar mass of substance (g/mol)
The molar mass of H2SO4 is:
(2 * atomic mass of H) + atomic mass of S + (4 * atomic mass of O)
= (2 * 1.008) + 32.07 + (4 * 16.00)
= 98.09 g/mol
Moles of H2SO4 = 150.0g / 98.09 g/mol
2. Use the mole ratio from the balanced equation to determine the moles of NaCO3 required:
The mole ratio between H2SO4 and NaCO3 is 1:1, so moles of NaCO3 = moles of H2SO4.
3. Finally, convert the moles of NaCO3 to the minimum number of sodium carbonate required:
Since 1 mole of NaCO3 is the minimum required, you can conclude that the minimum number of moles of NaCO3 needed is equal to the moles of H2SO4.
Therefore, the minimum number of moles of sodium carbonate (NaCO3) that have to be added to complete the reaction is equal to the calculated moles of H2SO4.