Aqueous sulfuric acid (H2SO4) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na2SO4) and liquid water (H2O). What is the theoretical yield of sodium sulfate formed from the reaction of 3.9 g of sulfuric acid and 1.8g of sodium hydroxide?

The theoretical yield of is, 5.65 grams.

Explanation : Given,

Mass of = 3.9 g

Mass of = 7.8 g

Molar mass of = 98 g/mol

Molar mass of = 40 g/mol

First we have to calculate the moles of and .

and,

Now we have to calculate the limiting and excess reagent.

The balanced chemical equation is:

From the balanced reaction we conclude that

As, 1 mole of react with 2 mole of

So, 0.0398 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of

From the reaction, we conclude that

As, 1 mole of react to give 1 mole of

So, 0.0398 mole of react to give 0.0398 mole of

Now we have to calculate the mass of

Molar mass of = 142 g/mole

Therefore, the theoretical yield of is, 5.65 grams.

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year