HNO3+FeO- Fe(NO3)3+NO+H2O

The reaction you provided is a redox reaction between nitric acid (HNO3) and iron(II) oxide (FeO). In this reaction, the iron(II) oxide is oxidized, and nitric acid is reduced, resulting in the formation of iron(III) nitrate (Fe(NO3)3), nitric oxide (NO), and water (H2O). Let's summarize the balanced reaction: **Unbalanced Reaction:** \[ \text{HNO}_3 + \text{FeO} \rightarrow \text{Fe(NO}_3\text{)}_3 + \text{NO} + \text{H}_2\text{O} \] **Balanced Reaction:** To balance this reaction, you will need to ensure that the number of atoms of each element is the same on both sides. 1. Count the number of each type of atom in the reactants and products. 2. Adjust the coefficients to balance the equation. The balanced reaction is: \[ 4 \text{HNO}_3 + 3 \text{FeO} \rightarrow 3 \text{Fe(NO}_3\text{)}_2 + 2 \text{NO} + 2 \text{H}_2\text{O} \] ### Important Notes: - In some contexts, the product of Iron(II) reacting with excess nitric acid can lead to the formation of iron(III) nitrate due to oxidation of Fe(II) to Fe(III). - In actual laboratory scenarios, the exact products can vary based on concentration and reaction conditions. - Always remember balancing chemical reactions includes ensuring both mass and charge are conserved.