Question

2.According to the following reaction, how many grams of dinitrogen monoxide will be formed upon the complete reaction of 28.0 grams of ammonium nitrate?

3.According to the following reaction, how many grams of hydrobromic acid are needed to form 25.4 grams of bromine

4For the following reaction, 3.96grams of chlorine gas are mixed with excess bromine . The reaction yields 11.3 grams of bromine monochloride . bromine ( g ) + chlorine ( g ) bromine monochloride ( g ) What is the theoretical yield of bromine monochloride ? grams What is the percent yield for this reaction ? %

5.For the following reaction, 5.34grams of iron(III) oxide are mixed with excess hydrochloric acid. The reaction yields 1.51 grams of water. hydrochloric acid (aq) + iron(III) oxide (s) water (l) + iron(III) chloride (aq) What is the theoretical yield of water ? grams What is the percent yield of water ?

6.For the following reaction, 6.41grams of carbon tetrachloride are mixed with excess methane (CH4) . The reaction yields 4.99 grams ofdichloromethane (CH2Cl2) . methane (CH4) ( g ) + carbon tetrachloride ( g ) dichloromethane (CH2Cl2) ( g ) What is the theoretical yield ofdichloromethane (CH2Cl2) ? grams What is the percent yield for this reaction ? %

7.How many milliliters of an aqueous solution of 0.196 M iron(III) chloride is needed to obtain 17.7 grams of the salt?

8.In the laboratory you dissolve 23.1 g of nickel(II) iodide in a volumetric flask and add water to a total volume of 375 . mL. What is the concentration of the nickel cation? What is the concentration of the iodide anion? What is the molarity of the solution? M 9.In the laboratory you dissolve 15.1 g of manganese(II) acetate in a volumetric flask and add water to a total volume of 500 mL. What is the molarity of the solution? What is the concentration of the manganese(II) cation? What is the concentration of the acetate anion?

10.In the laboratory you dissolve 19.6 g of iron(III) chloride in a volumetric flask and add water to a total volume of 500 mL. What is the molarity of the solution? M. What is the concentration of the iron(III) cation? M. What is the concentration of the chloride anion?

11.In the laboratory you dissolve 23.1 g of nickel(II) iodide in a volumetric flask and add water to a total volume of 375 mL. What is the molarity of the solution? What is the concentration of the nickel cation? What is the concentration of the iodide anion?

Answer 1

2. Reaction,

NH4NO3 ---> N2O + 2H2O

moles NH4NO3 = 28 g/80.04 g/mol = 0.35 mol

moles N2O formed = 0.35 mol

mass N2O formed = 0.35 mol x 44.0 g/mol = 15.4 g

3. for the reaction,

2HBr --> H2 + Br2

moles Br2 formed = 25.4 g/159.8 g/mol = 0.16 mol

moles HBr needed = 2 x 0.16 = 0.32 mol

mass HBr needed = 0.32 mol x 80.9 g/mol = 25.9 g

4. for the reaction,

Cl2 + Br2 --> ClBr

moles Cl2 present = 3.96 g/71 g/mol = 0.056 mol

Theoretical moles ClBr produced = 2 x 0.056 mol = 0.112 mol

theoretical mass of ClBr formed = 0.112 mol x 115.36 g/mol = 12.92 g

Percent yield = (11.3/12.92 ) x 100 = 87.46%

5. moles Fe2O3 taken = 5.34 g/159.7 g/mol = 0.0334 mol

Theoretical moles H2O produced = 3 x 0.0334 = 0.100 mol

theoretical yield of H2O = 0.100 mol x 18.01 g/mol = 1.81 g

percent yield of water = (1.51/1.81) x 100 = 83.58%