Chemistry Help? Balance the following equation representing a reaction that occurs in an acidic solution...?

Oxidation half equation: H₂O₂(aq) → 2H⁺(aq) + O₂(g) + 2e⁻
Reduction half equation: Cr₂O₇²⁻(aq) + 14H⁺(aq) + 6e⁻ → 2Cr³⁺(aq) + 7H₂O(ℓ)

(Oxidation half equation)×3 + (Reduction half equation)×1, and cancel 6e⁻ and 6H⁺ on each side.
The overall net ionic equation is:
3H₂O₂(aq) + Cr₂O₇²⁻(aq) + 8H⁺(aq) → 2Cr³⁺(aq) + 3O₂(g) + 7H₂O(ℓ)

Cr2O72- + 3 H2O2 + 8 H+ → 2 (Cr)3+ + 3 O2 + 7 H2O

there's your answer