Calculate the number of moles of NaOH that are needed to react with 500.0 g of H2SO4 according to the following equation:
H2SO4 + 2NaOH →
Na2SO4 + 2H2O

The number of mole of NaOH required to react with 500 g of H₂SO₄ is 10.2 moles

We'll begin by calculating the number of mole of in 500 g of H₂SO₄

Mole = mass / molar mass

Mole of H₂SO₄ = 500 / 98

Mole of H₂SO₄ = 5.1 moles

Finally, we shall determine the mole of NaOH required for the reaction.

H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

From the balanced equation above,

1 mole of H₂SO₄ required 2 moles of NaOH.

Therefore,

5.1 moles of H₂SO₄ will require = 5.1 × 2 = 10.2 moles of NaOH

Thus, 10.2 moles of NaOH is required for the reaction

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2.55 moles of NaOH are needed react with 500.0 gram of H₂SO₄.

Explanation:

Given data:

Mass of H₂SO₄ = 500.0 g

Number of moles of NaOH needed = ?

Solution:

H₂SO₄ + 2NaOH  → Na₂SO₄ + 2H₂O

Number of moles of H₂SO₄:

Number of moles = mass/molar mass

Number of moles = 500.0 g/ 98.07 g/mol

Number of moles = 5.09 mol

Now we will compare the moles of H₂SO₄ and NaOH.

                     H₂SO₄         :           NaOH

                           1             :               2

                         5.09         :            1/2×5.09 = 2.55 mol

Thus, 2.55 moles of NaOH are needed react with 500.0 gram of H₂SO₄.

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answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

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