according to the following reaction, how many moles of water are necessary to form 0.680 moles sulfurous acid (h2so3)?

sulfur dioxide (g) + water (l) sulfurous acid (h2so3) (g)

0.680 moles of water

Explanation:

Sulfurous acid is formed by the reaction of water and sulfur dioxide.

Balanced reaction will provide the basic information.

Balanced Reaction :

                          SO₂ +  H₂O > H₂SO₃

                         1 mol    1mol                  1mol

From above reaction we come to know

1 mole of H₂O ≅ 1 mole H₂SO₃

if 1 mole of H₂O produces 1 mole of H₂SO₃ then

0.680 mole of water will be required to produces sulfurous acid

Explanation through calculation

apply the unity formula

1 mole of the H₂O ≅ 1 mole of H₂SO₃

x mole of the H₂O ≅  0.680 moles of H₂SO₃

so by cross multiplication

1 mole  x X mole ≅ 1 mole  x 0.680 mole

we have to find moles of H₂O so by rearrangement of the above equation

X mole of H₂O = 1 mole x 0.680 mole

X mole of H₂O =  0.680 moles

since electrons are negative the answer is neagtaive

catya your not at all which answer i've seen you do this on another question!