1. At high temperatures, sulfur combines with iron to form the brown-black iron (II) sulfide: Fe (s) + S (l) ( FeS (s)
In one experiment, 7.62 g of Fe are allowed to react with 8.67 g of S. a. What is the limiting reagent, and what is the reactant in excess? b. Calculate the mass of FeS formed.
2. Arcylonitrile, C3H3N, is the starting material for the production of a kind of synthetic fiber acrylics) and can be made from propylene, C3H6, by reaction with nitric oxide, NO, as follows:
4 C3H6 (g) + 6 NO (g) → 4 C3H3N (s) + 6 H2O (l) + N2 (g)
What mass of C3H3N can be made when 21.6 g of C3H6 react with 21.6 g of nitric oxide?
3. Calculate the percent yield for the reaction: P4 (s) + 6 Cl2 (g) → 4 PCl3 (l) if 75.0 g of phosphorus reacts with excess chlorine gas to produce 111.0 g of phosphorus trichloride.
4. Formic acid, HCHO2, burns in oxygen to form carbon dioxide and water as follows:
HCHO2 (aq) + O2 (g) → 2 CO2 (g) + 2 H2O (l).
If a 3.15-g sample of formic acid was burned in 2.0 L of oxygen, what volume of carbon dioxide would be produced? (Assume the reaction occurs at standard temperature and pressure, STP.)
5. Zinc metal reacts with hydrochloric acid to produce zinc chloride and hydrogen gas. a. Balance the following reaction: Zn (s) + HCl (aq) → ZnCl2 (aq) + H2 (g) b. A 3.50-g sample of zinc metal is allowed to react with 2.50 g of hydrochloric acid.
Complete the following table:
|Reactants/products |Zn (grams) |HCl (grams) |ZnCl2 (grams) |H2 (L) | |Before reaction | | | | | |After reaction |1.26 g |...