Chem eq. + random word problems help?

Question

plz i really need help. just a few examples. i have like 200 more to do.. -_-

tell the type of reactions, predict the product write balancing equation and plz write the phase of the product. like x+y = X (solid). that kinda stuff.

1Ammonium sulfate reacts with barium nitrate,

2. Zinc metal is added to a solution of copper (II) chloride.

3. Propane gas (C3H8) is burned in excess oxygen.

4. Dinitrogen tetroxide gas is added to distilled water.

5. Solid calcium chlorate is heated strongly.

6. Sodium hydroxide solution is added to a solution of iron (III) bromide.

7. Chlorine gas is bubbled through a solution of sodium bromide.

8. Solutions of lead nitrate and calcium iodide are combined.

9. Sulfuric acid is combined with solid magnesium hydroxide.

10. Solid barium oxide is added to distilled water.

11. Isopropyl alcohol (C3H7OH) is burned in air.

12. Iron metal shavings are added to hydrochloric acid.

13. Solid sodium carbonate is heated in a crucible.

Answer 1

I don't want to do your homework for you, so I will only give a few equations.

1.  Know your solubility rules: barium sulfate is insoluble, thus, this is a double displacement reaction:

(NH4)2SO4(aq) + Ba(NO3)2(aq) -----> BaSO4(s) + 2NH4NO3(aq)

2. This is a redox reaction (single replacement).  Refer to the activity series of metals: zinc is more active than copper, so it will displace the copper from solution:

Zn(s) + CuCl2(aq) -----> ZnCl2(aq) + Cu(s)

3. This is a combustion reaction.  With an excess of oxygen, the propane will combust completely to form carbon dioxide (CO2) and water (H2O) and a lot of heat - both products will be produced as gases.

4. Most nonmetal oxides in water form acids.  N2O4 has N in the 4+ oxidation state, but there is no oxoacid of nitrogen with this oxidation state on the N.  Thus, it will disproportionate (some N atoms will get a different oxidation state) to form nitric acid (oxidation state of N is +5) and nitrous acid (oxidation state of N is +3):

N2O4(g) + H2O(l) ----> HNO3(aq) + HNO2(aq)

5.  This is a decomposition reaction.  Chlorine is very electronegative, but in this compound it is forced to assume a positive charge by the oxygen.  It is not very stable, so heating drives off oxygen gas, leaving behind the metal chloride.

6. Again, check your solubility rules - the ions can recombine to make iron(III) hydroxide and sodium bromide - are any of these insoluble?  If so, they will precipitate as solids.

7. Another single replacement reaction - this time with halogens instead of metals.  These also have an activity series: fluorine is the most electronegative, while iodine (well, really astatine, but this is too radioactive to care about) is the least.  Thus, elemental bromine, for example, will displace iodine from a solution with iodide ions, forming bromide ions and elemental iodine.  See if you can figure this one out for Cl2 and Br-...

8.Check those solubility rules again!

9. This is an acid-base reaction.  Sulfuric acid is a strong acid, while magnesium hydroxide is a weak base.  They will combine to form water and the magnesium salt of the acid:

H2SO4(aq) + Mg(OH)2 -----> MgSO4(aq) + 2H2O(l)

10.  Sort of like 4, but when some metal oxides (those of alkali metals, Ca, Sr, and Ba) are added to water, they become hydroxides (bases) instead of acids:

BaO(s) + H2O(l) -----> Ba(OH)2(aq)

11. Another combustion reaction.  Don't let the oxygen already in the molecule fool you - you'll just need to add a little bit less oxygen to react all of the carbon to form CO2 and all of the hydrogen and oxygen to form water.

12. Another single replacement (redox) reaction.  Hydrogen isn't a metal, but behaves enough like one in solution that it can be treated as such for these problems.  Hydrogen is below iron on the activity series, so the iron will reduce the hydrogen ions from the acid to H2 gas.

13. Another decomposition.  When you have a polyatomic ion with a nonmetal and oxygen in it, its salts will almost always decompose to make the nonmetal oxide and the oxide of the metal in the salt.  The exception is when the nonmetal is a halogen, as in 5.  So this reaction will form solid sodium oxide and carbon dioxide gas.