insert the missing coefficients in the following partially balanced chemical equations S+6HNO=HSO4+NO+H2O

S + 6HNO₃ ⟶ H₂SO₄ + 6NO₂ + 2H₂O

Step-by-step explanation:

S + 6HNO₃ ⟶ H₂SO₄ + NO₂ + H₂O

One way is to balance this equation is the oxidation number method.

Step 1. Calculate the oxidation number of every atom:

S⁰ + H⁺¹N⁺⁵O₃⁻² ⟶ H₂⁺¹S⁺⁶O₄⁻² + N⁺⁴O₂⁻² + H₂⁺¹O⁻²

Step 2. Identify the changes in oxidation number:

S: + 0 ⟶ + 6; Change = + 6

N: + 5 ⟶ + 4; Change = - 1

Step 3. Equalize the changes in oxidation number.

You need 6 atoms of N for every 1 atom of S. This gives us total changes of - 6 and + 6.

Step 4. Insert coefficients to get these numbers.

1S + 6HNO₃ ⟶ 1H₂SO₄ + 6NO₂ + H₂O

Step 5. Balance O.

We have fixed 18 O on the left and 16 O on the right. We need 2 more O on the right. Put a 2 in front of H₂O.

1S + 6HNO₃ ⟶ 1H₂SO₄ + 6NO₂ + 2H₂O

Every formula now has a coefficient. The equation should be balanced.

Step 6. Check that all atoms balance.

Atom Left-hand side Right-hand side

S 1 1

H 6 6

N 6 6

O 18 18

The balanced equation is

S + 6HNO₃ ⟶ H₂SO₄ + 6NO₂ + 2H₂O