Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. Although you can write a balanced equation using only 2 moles of nitric per mole of zinc, in reality, some of the nitric is lost in oxidixing the zinc and thus reducing some of the NO2 to NO. Denis M is absolutely correct. Question: QUESTION 3 Consider The Reaction Between Zinc And Nitric Acid. Zn + 2 HNO3 (dilute) ---> Zn(NO3)2 + H2 Concentrated nitric acid on the other hand is a powerful oxidising agent, and Calculate the number of grams of zinc that must react with an excess of HNO3 to form 29.1g NH4 NO3. Nitric acid can be reacted with zinc according to the following chemical equation.

Actually, zinc ions are formed and the nitrate ions are left over from the nitric acid (which dissociates into ions in water The products formed when zinc reacts with dilute nitric acid are zinc nitrate and hydrogen gas; i.e. If You Were Asked To Perform This Chemical Reaction What Would You Observe? Ans: Zinc reacts with dilute Nitric acid to produce Zinc nitrate, nitric oxide and water 3Zn + 8HNO₃ → 3Zn(NO₃)₂ + 2NO + 4H₂O Zinc reacts with concentrated Nitric acid to produce Zinc nitrate, nitrogen dioxide and water. How many atoms of zinc react with 1.49g HNO3? 4HNO3(aq) + Zn(s) → Zn(NO3)2(aq) + 2H2O(1) + 2NOz (9) If 1.65 g of Zn is added to 165 mL of 0.110 M HNO3, what mass of NO2 would be produced In the balanced equation above you see Zn(NO3)2(aq), and we might say that zinc nitrate is the product. How do I balance the reaction equation of zinc and nitric acid?