Write balanced chemical equations for the following reactions. For EACH chemical, write the coefficient in the first box, the chemical in the second box, and the state in the third box. Do not use subscripts or superscripts in your answer: for example, Caz(PO4)2 would be entered "Ca3(PO4)2". Solutions of iron (II) sulfate and calcium chloride react. iron reactant calcium reactant iron product calcium product

Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction.   NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g)  Balance the reaction.

Select all of the ions that are spectator ions in the below chemical reaction. Incorrect selections will deduct credit. 3 MgBr2 (aq) + 2 NazPO4 (aq) → Mg3(PO4)2 (s) + 6 NaBr (aq) Na+ PO,3- Br Mg2+ O There are no spectator ions.

10. The equations below represent precipitation reactions. Rewrite these as complete ionic and net ionic equations. Molecular Equation Complete Ionic Equation Net Ionic Equation Molecular Equation Complete lonic Equation Net Ionic Equation AgNO, (aq) + KCI (og) → KNO, (aq) + AgCl (s) Molecular Equation Complete Ionic Equation Net Ionic Equation Ba(ClO4)2 (aq) + K₂SO4 (ng) BaSO (s) + 2 KCIO₂(g) 11. The equation below represents a neutralization reaction. Rewrite this as complete ionic equations and net ionic equations. 2 HCl(aq) + Ba(OH)2 (aq) → 2 H₂O )+ BaCl₂ (aq) Include phase symbols.

Write the balanced precipitation reactions

6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)

1. Label each of the following reactions as combination (synthesis), decomposition, single replacement, or double replacement. Then complete and balance the following reactions. Reaction Type of reaction? Redox or nonredox? H2(g) + 02 (g) → K (s) + N2 (g) → C (s) + 02 (g) → H2CO3 (aq) → electrical current H₂O (1) 300°C Au2O3 (s) 300°C Ag2O (s) → NH3 (g) → Pb (s) + Cu(NO3)2 (aq) → Na (s) + HOH (1) -> BaBr2 (aq) + Na3PO4 (aq) → H2SO4 (aq) + NH4OH(aq) → Cl2 (g) + NaI (aq) → Na2S (s) + HCl(aq) → Fe (s) + 02 (g) →

Balance the following reaction in basic solution then enter the coefficients of the balanced reaction into the blank spaces. Remember to include "understood" coefficients of 1! 9. Type your answer here Ag20(s) + Type your answer here Al(s) + Type your answer here OH (aq) + H20(1) → Type your answer here Type your answer here Ag(s) + Type your answer here H2A!O3 (aq)

Cobalt(II) chloride solution reacts with sodium hydroxide solution. Identity the spectator ion(s). Note: you may choose more than one answer. O Co2+ Na OH

Here is some information to help. In this experiment, magnesium metal is heated until it reacts with oxygen in the air according to the following balanced equation: 2Mg(s)+ O2(g) → 2MgO(s)                                                                  (silver metal)                  (white-gray ash) As the magnesium burns in air, it may also combine with nitrogen in air. To remove any nitride product, water is added, and the product is reheated. Any nitride product is converted to magnesium oxide and ammonia. 3Mg(s)+ N2(g) → Mg3N2(s) Mg3N2(s)+3H2O(l)→3MgO(s)+2NH3(aq) A weighed amount of the magnesium metal is used, and the mass of the oxide product formed is determined at the end of the experiment. The mass of oxygen that combines with the magnesium is obtained from the difference between the mass of the oxide product and the original mass of magnesium. mass of oxide product-mass of magnesium=mass of oxygen in oxide product The empirical formula of the oxide…