How many miles of sodium hydrogen carbonate would be needed to react with 150.0 g of sulferic acid?
Kindly tell me what miles of NaHCO3 are?
1. Write the balanced equation.
2NaHCO3 + H2SO4 ==> Na2SO4 + 2H2O + 2CO2
2. Convert 150 g H2SO4 to moles. moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles (you must have meant moles instead of miles) H2SO4 to moles NaHCO3. And you're done.
To determine the number of miles of sodium hydrogen carbonate required to react with 150.0 g of sulfuric acid, we need to use stoichiometry. Stoichiometry is a mathematical relationship between the amounts of reactants and products in a chemical reaction.
Step 1: Write the balanced equation for the reaction between sulfuric acid (H2SO4) and sodium hydrogen carbonate (NaHCO3):
H2SO4 + 2NaHCO3 -> Na2SO4 + 2H2O + 2CO2
This equation tells us that one mole of sulfuric acid reacts with two moles of sodium hydrogen carbonate to produce one mole of sodium sulfate, two moles of water, and two moles of carbon dioxide.
Step 2: Determine the molar mass of sulfuric acid:
H2SO4: (2 x 1.01 g) + (1 x 32.07 g) + (4 x 16.00 g) = 98.09 g/mol
Step 3: Convert the mass of sulfuric acid to moles:
Moles of H2SO4 = Mass of H2SO4 / Molar mass of H2SO4
Moles of H2SO4 = 150.0 g / 98.09 g/mol ≈ 1.53 mol
Step 4: Use stoichiometry to calculate the moles of sodium hydrogen carbonate needed:
From the balanced equation, we can see that 1 mole of sulfuric acid reacts with 2 moles of sodium hydrogen carbonate.
Therefore, moles of NaHCO3 = (1.53 mol H2SO4) x (2 mol NaHCO3 / 1 mol H2SO4) = 3.06 mol
Step 5: Convert the moles of sodium hydrogen carbonate to mass:
Mass of NaHCO3 = Moles of NaHCO3 x Molar mass of NaHCO3
Mass of NaHCO3 = 3.06 mol x 84.01 g/mol = 257.03 g
Step 6: Convert the mass of sodium hydrogen carbonate to miles:
To convert grams to miles, we need to know the density of sodium hydrogen carbonate in g/mile. Without this information, we cannot directly convert grams of sodium hydrogen carbonate to miles.