1.
What is the empirical formula of a compound with the following
percentages: 30.46% Nitrogen and 69.54% Oxygen.
2.
A blue solid is found to contain 36.84% nitrogen and 63.16% oxygen.
What is the empirical formula for this solid?
3.
A compound was found to contain 49.98g carbon and 10.47g
hydrogen. The molar mass of the compound is 58.14g/mole.
Determine the molecular formula.
4.
Chloroform (CHCl3), an important solvent, is produced by a reaction
between methane and chlorine.
CH4 (g) + Cl2 (g) → CHCl3 (g) + HCl (g)
How many grams of CH4 is needed to produce 50g of CHCl3?
5.
The reaction of chlorine gas with solid phosphorous (P4) produces
solid phosphorous pentachloride. When 16g of chlorine reacts with
23g P4 , which reactant limits the amount of phosphorous
pentachloride produced?
Cl2 + P4 → PCl5
6.
Analysis of a compound indicates that it contains 1.04g K, 0.70g Cr,
and 0.86 g O. Find its empirical formula.
7.
Monosodium glutamate (MSG) is sometimes added to food to
enhance flavor. Analysis determined this compound to be 35.5% C,
4.77% H, 8.29% N, 13.6% Na and 37.9% O. What is the empirical
formula for MSG?
8.
CaCo3(s) + H2CO3(aq) → Ca(HCO3)2(aq)
250g of CaCo3 will produce how many grams of Ca(HCO3)2?
9.
Zn(s) + MnO2(s) + H2O(l) → Zn(OH)2 + Mn2O3
Determine the limiting reactant if 25g Zn and 30g MnO2 are reacted.
10. Glycerol is a thick, sweet liquid obtained as a by product of the
manufacture of soap. Its percent composition is 39.12% carbon,
8.75% hydrogen, and 52.12% oxygen. The molar mass is 92.11
g/mole. What is the molecular formula for glycerol?
11. One in a series of reactions that inflate air bags in automobiles is the
decomposition of sodium azide (NaN3). Determine the mass of N2
produced if 100.0g of NaN3 is decomposed.
NaN3(s) → Na(s) + N2
12. How many grams of hydrogen are necessary to react with sufficient
chlorine to produce 45.7 grams of hydrogen chloride?
H2 + Cl2 → HCl
13. How many grams of cesium xenon heptafluoride (CaXeF7) can be
produced from the reaction of 12.5 grams of cesium fluoride with
10.5 grams of xenon hexafluoride?
CsF(s) + XeF6(s) → CsXeF7(s)
14. If 4.04g of N combine with 11.46 g O to produce a compound with a
formula mass of 108.0 g/mole, what is the molecular formula of this
compound?
15. Silicon dioxide (quartz) is usually quite unreactive but reacts readily
with hydrogen fluoride according to the following equation:
SiO2 + HF → SiF4 + H2O
What is the limiting reactant if 118.3 g of SiO2 are exposed to 120.2 g
of HF? (Use water as your question mark)
16. The molar mass of a compound is 92 g/mole. Analysis of a sample of
the compound indicates that it contains 0.606 g N and 1.390 g O.
Find its molecular formula.
17. Determine the molecular formula for ibuprofen, a common headache
remedy. Analysis of ibuprofen yields a molar mass of 206 g/mole and
a percent composition of 75.7% C, 8.80% H, and 15.5% O.
18. What is the empirical formula of a compound that contains
10.52 g Ni, 4.38 g C, and 5.10 g N.
19. The reaction between solid sodium and iron (III) oxide is one in a
series of reactions that inflates an automobile airbag.
Na + Fe2O3 → Na2O + Fe
20. Ammonium nitrate (NH4NO3), an important fertilizer, produces N2O
gas and H2O when it decomposes. Determine the mass of water
produced from the decomposition of 25.66 g of solid ammonium
nitrate.
NH4NO3 → N2O + H2O