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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

antiseptic1488 [7]

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 (n = mass/molar mass).

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.

Using cross multiplication:

1.0 mole of H₂SO₄ → 2.0 moles of H₂O, from the stichiometry of the balanced equation.

??? moles of H₂SO₄ → 3.1666 moles of H₂O.

The number of moles of H₂SO₄ that will produce 3.1666 moles of H₂O (57.0 g) is (1.0 x 3.1666 / 2.0) = 1.5833 moles.

Finally, we should convert the number of moles of H₂SO₄ into grams (n = mass/molar mass).

Molar mass of H₂SO₄ = 98.0 g/mole.

mass = n x molar mass = (1.5833 x 98.0) = 155.16 g.

6 0

3 years ago

Read 2 more answers

What is 6.9 x 10^-3 in standard form?

Maslowich

Answer:

0.0069

Explanation:

When converting between scientific notation try to remember that moving the decimal place to the left is positve and to the right is negative

Since you are changing from scientific to standard you will need to move to the left from the decimal point, making your answer 0.0069

4 0

2 years ago

A chemistry student needs of acetic acid for an experiment. He has available of a w/w solution of acetic acid in acetone. Calcul

Volgvan

Answer:

49.4 g Solution

Explanation:

There is some info missing. I think this is the original question.

A chemistry student needs 20.0g of acetic acid for an experiment. He has 400.g available of a 40.5 % w/w solution of acetic acid in acetone.

Calculate the mass of solution the student should use. If there's not enough solution, press the "No solution" button. Round your answer to 3 significant digits.

We have 400 g of solution and there are 40.5 g of solute (acetic acid) per 100 grams of solution. We can use this info to find the mass of acetic acid in the solution.

$400gSolution \times \frac{40.5gSolute}{100gSolution} = 162 g Solute$