Question

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)

Answer 1

0.680 moles of water

Step-by-step 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