Aqueous sulfuric acid reacts with solid sodium hydroxide to produce aqueous sodium sulfate and liquid water . What is the theoretical yield of sodium sulfate formed from the reaction of of sulfuric acid and of sodium hydroxide

71g (assuming experimental data)

Explanation:

The balanced equation for this reaction:

+ → +

Molar mass of H2SO4 = 98.1 g/mol

molar mass of NaOH = 40g/mol

Molar mass of Na2SO4 = 142.04g/mol

⇒ 1 mole or 98.1g of H2SO4 will yield 1 ole of NaSO4; alternately, 2 moles or 49 ×2 = 80g of NaOH produces 1 mole of NaSO4.

Therefore, limiting reactant is NaOH.

Assuming actual experiment is 20g of NaOH,

1 mole - 40g

x moles - 20g = = 0.5 moles

⇒1 mole of Na2SO4 - 142.04g

∴ 0.5 moles = 142.04 × 0.5

= 71.02g

what is the volume occupied by 40 grams of argon gas (ar) at standard conditions? what volume, in liters, is occupied by 1.5 x 1023 

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots