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25 Empirical Formula, Stoichiometry and Redox Problems

1.)A hydrocarbon has the formula C12H20. 61.51 g of it are burned in the presence of excess pure oxygen gas. How many grams of water are produced in this combustion?

Use these atomic weights: 12.01(C), 1.008(H), and 16.00(O).

2.)How many mL of water are needed to dilute 32.07 mL of a solution 1.53 M in HCl to 0.154 M HCl?

3.): What is the oxidizing agent in the following REDOX reaction?
Zn(s) + Cu2+(aq) ===> Cu(s) + Zn2+(aq)

4.)The cyanide ion, CN-, has many of the properties of halide ions. On this basis, you would expect it to form a precipitate with the Na+ cation
true or false?

5.)The cyanide ion, CN-, has many of the properties of halide ions. On this basis, you would expect it to form a precipitate with the Ag+ cation.
true or false?

6.)Using the following portion of the activity series for oxidation half reactions, determine which reaction will occur:
K ===> K+ + e-
Al ===> Al3+ + 3e-
Fe ===> Fe2+ + 2e-
Sn ===> Sn2+ + 2e-
(Assume aqueous solution. I have left out the (s) and (aq) symbols.)

8.)In the balanced equation for the reaction where dichromate oxidizes aq. HCl to chlorine gas, the number of waters is (acidic solution)...

9.)Which of the following compounds is an Arrhenius base?
CH3OH
CH3COOH
HOCl
KOH

10.)which of these are cations which are precipitated by the chloride anion.
Ag+
H+
Ba2+
Na+
NH4+

11.)How many sulfur atoms are in 35.0 g of aluminum sulfide?

13.)Which of the following compounds has the highest percentage of carbon by mass?
CH3COOOH
C2H5OH
C2H6
CaC2
H2C2O4

14.)How many moles of NaOH are in 22.0 mL of 0.150M NaOH?

15.)The formula for zirconium phosphate is Zr3(PO4)4. On the basis of this information, the formula for the sulfide of Zr would be expected to be

16.)Which of the following samples contains the largest number of atoms?
1.0 mol propane gas, C3H8
5.0 mol iodine vapor, I2
2.5 mol ammonia, NH3
10.0 mol neon gas, Ne
3.0 mol water

17.)Write a balanced equation for the combustion of butane, C4H10. The coefficient of oxygen in the balanced equation is.

18.)Chlorine was passed over 1.10 g of heated titanium and 3.54 g of a chloride of Ti were obtained. What is the empiricial formula of this chloride?

19.)Tartaric acid, which occurs in many fruits, has MW = 150.1 and contains 63.96% oxygen by mass. How many oxygen atoms are in each tartaric acid molecule?

20.)formula weight of aluminum sulfate to the nearest 0.01 g/mol
Al2 (SO4)3 MW = 342.17 g/mol

21.)Which of the following contains the greatest mass of oxygen?
1.0 mol O2
1.0 mol ozone (O3)
1.0 mole potassium chlorate
0.50 mol potassium dichromate
0.50 mol Na2S2O8

22.)The analysis of an organic compound showed that it contains 0.175 mol of C, 0.140 mol of H, and 0.0350 mol of N. Its molecular mass is about 160. How many atoms of carbon are there in the empirical formula and the molecular formula, respectively?

23.)The total number of atoms in one formula unit of ferric sulfate is?

24.)An organic compound which has the empirical formula CHO has an approximate molar mass of 145 g/mol. The best guess at its molecular formula is
C2H2O2
C3H3O3
C4H4O4
C5H5O5
C6H6O6

25.)250.0 mL of 3.00 M HCl are added to 400.0 mL of 6.00 M HCl. Assuming that the volumes are additive, the final concentration is

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An assortment of detailed solutions to 25 empirical formula, stoichiometry and redox problems.

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