If 150.0 f of sulfuric acid is spilled, what is the minimum number of moles of sodium carbonate have to be added to complete reaction
always start with the balanced equation.
Na2CO2+H2SO4>>Na2SO4 + CO2 + H2O
so the number of moles of sodium carbonate is the same number of moles of sulfuric acid.
So you need to know the moles of H2SO4, I am uncertain what 150 f of..means
Yes the 150f is confusing. Pls throw more light on it
To find the minimum number of moles of sodium carbonate required to complete the reaction with 150.0 grams of sulfuric acid, we need to determine the stoichiometry of the reaction between sulfuric acid (H2SO4) and sodium carbonate (Na2CO3).
The balanced chemical equation for the reaction between sulfuric acid and sodium carbonate is as follows:
H2SO4 + Na2CO3 -> Na2SO4 + CO2 + H2O
From this equation, we can see that one mole of sulfuric acid reacts with one mole of sodium carbonate to form one mole of sodium sulfate, one mole of carbon dioxide, and one mole of water.
To convert grams of sulfuric acid to moles, we need to calculate the molar mass of sulfuric acid (H2SO4). The molar mass of H2SO4 is calculated as:
2(1.008 g/mol) + 32.06 g/mol + 4(16.00 g/mol) = 98.09 g/mol
Now, we can calculate the number of moles of sulfuric acid:
moles of H2SO4 = mass of H2SO4 / molar mass of H2SO4
= 150.0 g / 98.09 g/mol
≈ 1.528 moles
Since the stoichiometric ratio between sulfuric acid and sodium carbonate is 1:1, the minimum number of moles of sodium carbonate required will be approximately 1.528 moles.