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Write balanced chemical equations for the following reactions. Use ionic equations if appropriate, and consult the activity series of metals where...
Write balanced chemical equations for the following reactions. Use ionic equations if appropriate, and consult the activity series of metals where necessary. If there is no reaction, indicate this, and justify.
1. Ammonia is bubbled into nitrous acid. A neutral gas is released. Careful evaporation of the resulting solution leaves no residue.
2. Magnesium metal is burned in pure nitrogen.
3. Solutions of ammonium sulfate and barium hydroxide are mixed and heated. A white precipitate is formed, and a gas (which turns litmus blue) is released.
4. Calcium nitride is dissolved in hydrochloric acid. There is no precipitate formed, nor is any gas released.
5. Ammonia is bubbled into perchloric acid.
6. Sodium amide is added to dilute perchloric acid.
7. When solutions of sodium amide and ammonium nitrate (both in liquid ammonia) are mixed, the temperature increases and there is a large decrease in conductivity.
8. Aqueous ammonia is added to a solution of iron(III) nitrate. A rust-colored precipitate forms.
9. When aqueous solutions of hydrazine and hydrofluoric acid are mixed, there is a sharp increase in conductivity.
10. Hydrazine and a solution of iodic acid (HIO3) are mixed. A colorless gas is released, and the resulting solution is colorless. (Caution, balancing this one is difficult.)
Representative Syntheses:
A. Convert N2* to N*H3(g) (* indicates stable isotope 15N)
B. Convert NH3 and KNO2 to Ca3N2
C. Convert HNO3 to N2O(g)
