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Ivan
3 years ago
13

How many grams of sulfuric acid are needed to produce 57.0 grams of water? Show all steps of your calculation as well as the fin

al answer.
2NaOH+H2SO4 > 2Na2SO4+2H2O
Chemistry
2 answers:
antiseptic1488 [7]3 years ago
6 0

Answer:

155.16 g.

Explanation:

  • Firstly, It is considered as a stichiometry problem.
  • From the balanced equation: 2NaOH + H₂SO₄ → 2Na₂SO₄ + 2H₂O
  • It is clear that the stichiometry shows that 2.0 moles of NaOH reacts with 1.0 mole of H₂SO₄ to give 2.0 moles of Na₂SO₄ and 2.0 moles of H₂O.
  • We must convert the grams of water (57.0 g) to moles <em>(n = mass/molar mass)</em>.
  • n = (57.0 g) / (18.0 g/mole) = 3.1666 moles.
  • Now, we can get the number of moles of H₂SO₄ that is needed to produce 3.1666 moles of water.
  • <em>Using cross multiplication:</em>
  • 1.0 mole of H₂SO₄ → 2.0 moles of H₂O, <em>from the stichiometry of the balanced equation</em>.
  • ??? moles of H₂SO₄ → 3.1666 moles of H₂O.
  • The number of moles of H₂SO₄ that will produce 3.1666 moles of H₂O <em>(57.0 g)</em> is (1.0 x 3.1666 / 2.0) = 1.5833 moles.
  • Finally, we should convert the number of moles of H₂SO₄ into grams <em>(n = mass/molar mass)</em>.
  • Molar mass of H₂SO₄ = 98.0 g/mole.
  • mass = n x molar mass = (1.5833 x 98.0) = 155.16 g.
Sergeu [11.5K]3 years ago
5 0

<u>Answer:</u> 155.134 grams of sulfuric acid is needed.

<u>Explanation:</u>

To calculate the moles, we use the following equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of water:

Given mass of water = 57 grams

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

\text{Number of moles}=\frac{57g}{18g/mol}=3.166moles

For the given chemical reaction, the equation follows:

2NaOH+H_2SO_4\rightarrow 2Na_2SO_4+2H_2O

By Stoichiometry of the reaction:

2 moles of water are produced by 1 mole of sulfuric acid

So, 3.166 moles of water will produced by = \frac{1}{2}\times 3.166=1.583moles of sulfuric acid.

Now, to calculate the mass of sulfuric acid, we use the moles equation:

Molar mass of sulfuric acid = 98 g/mol

Putting values in above equation, we get:

1.583mol=\frac{\text{Given mass}}{98g/mol}

Mass of sulfuric acid = 155.134 grams

Hence, 155.134 grams of sulfuric acid is needed.

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