Practice Problems set: Set #3 IIa) Balance the following equations:(10 ...
Practice Problems set: Set #3
IIa) Balance the following equations:(10) 1) Zn (s) +
H3PO4 (aq) Zn3(PO4)2 (s) + H2(g)
2. Mg3N2 (s) + H2O (l) NH3(g) + Mg(OH)2 (s)
3. KMnO4(aq) + HCl(aq) Cl2 (g) + MnO2(s) + KCl(aq) + H2O(l)
4. NH3(g) + O2 (g) NO(g) + H2O (l)
5. Al2S3 (s) + H2O (l) Al(OH)3 + H2S(g)
IIb) Write a balanced chemical equation for each of the following:(8) 1. Solid copper reacts with solid sulfur to form solid copper(I) sulfide.
2. Solid magnesium reacts with aqueous copper (I) nitrate to form aqueous magnesium nitrate and solid copper.
3. Gaseous dinitrogen pentoxide decomposes to form nitrogen dioxide and oxygen gas.
4. Aqueous hydrochloric acid reacts with solid manganese (IV) oxide to form aqueous manganese (II) chloride, liquid water, and chlorine gas.
IIIa) Write the chemical formula for each of the following(5)
1.Potassium Dichromate
2. ammonium phosphate
3. Phosphoric acid
4. Baking Soda
5. Iron (III) sulfide
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Multiple Choice: 1. The balanced equation 2Cu(s) + O2 (g) 2CuO(s) tells us that 1 mol of Cu A. B. C. D. E.
reacts with 1 mol of O2 produces one mol of CuO must react with 32g of O2 cannot react with oxygen produces 2 mol of CuO
2. A 3.0 mol sample of KClO3 was decomposed according to the equation 2KClO3(s) 2KCl(s) + 3O2 (g) How many moles of O2 are formed assuming 100% yield?
A. B. C. D. E.
2.0 mol 2.5 mol 3.0 mol 4.0 mol 4.5 mol
3. What mass of carbon dioxide would be produced when 10.0 g of butane reacts with an excess of oxygen in the following reaction? 2C4H10(g) + 13 O2 (g) 8CO2 (g) + 10 H2O(g) A. B. C. D. E.
7.57g CO2 30.3g CO2 40.0g CO2 352g CO2 none of these
4. How many molecules of carbon dioxide would be formed if 6.75g of propane is burned in the following reaction? C3H8 (g) + 5O2 (g) 3 CO2 (g) + 4H2O (g) A. B. C. D. E.
5.54 x 1.39 x 20.3 x 2.77 x 3.89 x
1023 molecules 1023 molecules 1023 molecules 1023 molecules 1023 molecules
5.
Consider the following reaction:
2A
+ B 3C + D
3.0 mol A and 2.0 mol B react to form 4.0 mol C. What is the percent yield of the reaction? A. B. C. D. E.
50% 67% 75% 89% 100%
6. When NH3 is prepared from 28g N2 and excess H2, the theoretical yield of NH3 is 34g. When this reaction is carried out in a given experiment, only 30g is produced. What is the percentage yield?
A. B. C. D. E.
6% 12% 14% 82% 88%
7. The empirical formula for the compound having the formula H2C2O4 is A. B. C. D. E.
COH COH2 C2H2 C2O4H2 CO2H
8. Which of the following has the largest percent by mass of carbon? A. CaCO3 B. CO2 C. CH4 D. NaHCO3 9. A compound is analyzed and found to contain 12.1% carbon, 16.2% oxygen, and 71.7% chlorine (by mass). Calculate the empirical formula of this compound. A. COCl B. COCl2 C. CO2Cl D. CO2Cl2 E. COCl4
10. Calculate the molecular formula of a compound with the empirical formula CH2O and a molar mass of 150g/mol. A. B. C. D. E.
C2H4O2 C3H6O3 C4H8O4 C5H10O5 C6H12O6
11. A certain compound is found to have the percent composition (by mass) of 85.63% C and 14.37% H. The molar mass of the compound was found to be 42.0 g/mol. Calculate the empirical and the molecular formulas. A. B. C. D. E.
C2H3 and C4H6 CH and C3H3 CH2 and C3H6 CH3 and C2H6 C2H6 and C3H9
12. The correct formula for arsenic(III) oxide is A. B. C. D. E.
As3O3 As2O3 As3O2 AsO As3O 13 . Identify the incorrect statement among the following:
A. A mole is that quantity of a substance that contains 6.02x1023 particles of that substance. B. One mole of any substance contains the same number of particles as one mole of any other substance. C. One mole of any substance contains the same number of particles as the number of atoms in exactly 12 grams of carbon-12. D. A mole is a quantity of a substance that has a mass of exactly 12 grams. E. All of the above are correct.
14. In the sum of 54.34 + 45.66, the number of significant figures is A. B. C. D.
2 3 4 5
E. 6
15. The number 0.005802 expressed in scientific notation is A. B. C. D. E.
5.82 x 103 5.802 x 103 5.82 x 10-3 5.802 x 10-3 5802 x 10-6
16. Which of the following is a binary compound? A. O2 B. HCN C. H2SO4 D. H2S E. NaOH
17. Select the correct statement about
43
Ti
A. The nucleus contains 22 protons and 26 neutrons, mass number =48 B. The nucleus contains 22 protons and 21 neutrons, atomic number =22 C. The nucleus contains 21 protons and 22 neutrons, mass number =43. D. The nucleus contains 22 protons and 43 neutrons, atomic number 22 E . None of the above are correct.
18. The sum of the coefficients when the following equation is balanced is BaSO4 + K3PO4 a3 (PO4)2 + A. 4 A. B. C. D.
7 8 9 11
K2SO4
19. The name for HBrO (aq) is A. B. C. D. E.
hydrogen bromous acid bromous acid bromic acid hypobromous acid perbromic acid
20. The reaction AgNO3 (aq) + NaCl (aq) AgCl(s) + NaNO3(aq) is a(n) ------------------ reaction.
A. B. C. D. E.
precipitation acid-base oxidation-reduction none of these single replacement
21. A reaction that involves a transfer of electrons is called a(n) ------- reaction A. B. C. D. E.
precipitation acid –base oxidation-reduction double displacement none of these
IIb) Write a balanced chemical equation for the following: (4) 1. Aqueous hydrochloric acid reacts with solid manganese (IV) oxide to form aqueous manganese (II) chloride, liquid water, and chlorine gas.
2. Liquid nitric acid decomposes to reddish brown nitrogen dioxide gas, liquid water, and oxygen gas. (This is why bottles of nitric acidbecome yellow upon standing).
IIIa) Balance the following chemical equations.(6)
Na2O2(s) + H2O(l) NaOH(aq) + O2(g)
Mg3N2 (s) + H2O (l) NH3(g) + Mg(OH)2 (s)
FeCl3(aq) + KOH (aq) Fe (OH)3 + KCl (aq)
IIIb) Give the name and calculate the molar mass for each of the following:(4) 1.Cr2O3
2. NaOCl
IV)Solve the following: 1.Calculate the theoretical yield of NO and the percentage yield of NO if 49.2g of NO2 yield 8.90 grams of NO in the following reaction:(3 points) 3NO2(g) + H2O (g) 2HNO3(g) + NO(g)
2. Nitrogen gas can be prepared by passing gaseous ammonia over solid copper (II) oxide at high temperatures. The products of the reaction are solid copper and water vapour. How many grams of nitrogen are formed when 18.1g of NH3 are reacted with with 90.4g of CuO? (5 points)
BONUS QUESTION (6 points) Finish the following table. (Use the periodic chart given to you) Nuclear Symbol
# of Protons
34
-----------
S
-----------
23
------------
---------
# of Neutrons
---------------
28
-------------
# of electrons
-------------
------------
Atomic #
------------
------------
13
Mass #
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27
IIa) Balance the following equations:(10) 1) Zn (s) +
H3PO4 (aq) Zn3(PO4)2 (s) + H2(g)
2. Mg3N2 (s) + H2O (l) NH3(g) + Mg(OH)2 (s)
3. KMnO4(aq) + HCl(aq) Cl2 (g) + MnO2(s) + KCl(aq) + H2O(l)
4. NH3(g) + O2 (g) NO(g) + H2O (l)
5. Al2S3 (s) + H2O (l) Al(OH)3 + H2S(g)
IIb) Write a balanced chemical equation for each of the following:(8) 1. Solid copper reacts with solid sulfur to form solid copper(I) sulfide.
2. Solid magnesium reacts with aqueous copper (I) nitrate to form aqueous magnesium nitrate and solid copper.
3. Gaseous dinitrogen pentoxide decomposes to form nitrogen dioxide and oxygen gas.
4. Aqueous hydrochloric acid reacts with solid manganese (IV) oxide to form aqueous manganese (II) chloride, liquid water, and chlorine gas.
IIIa) Write the chemical formula for each of the following(5)
1.Potassium Dichromate
2. ammonium phosphate
3. Phosphoric acid
4. Baking Soda
5. Iron (III) sulfide
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Multiple Choice: 1. The balanced equation 2Cu(s) + O2 (g) 2CuO(s) tells us that 1 mol of Cu A. B. C. D. E.
reacts with 1 mol of O2 produces one mol of CuO must react with 32g of O2 cannot react with oxygen produces 2 mol of CuO
2. A 3.0 mol sample of KClO3 was decomposed according to the equation 2KClO3(s) 2KCl(s) + 3O2 (g) How many moles of O2 are formed assuming 100% yield?
A. B. C. D. E.
2.0 mol 2.5 mol 3.0 mol 4.0 mol 4.5 mol
3. What mass of carbon dioxide would be produced when 10.0 g of butane reacts with an excess of oxygen in the following reaction? 2C4H10(g) + 13 O2 (g) 8CO2 (g) + 10 H2O(g) A. B. C. D. E.
7.57g CO2 30.3g CO2 40.0g CO2 352g CO2 none of these
4. How many molecules of carbon dioxide would be formed if 6.75g of propane is burned in the following reaction? C3H8 (g) + 5O2 (g) 3 CO2 (g) + 4H2O (g) A. B. C. D. E.
5.54 x 1.39 x 20.3 x 2.77 x 3.89 x
1023 molecules 1023 molecules 1023 molecules 1023 molecules 1023 molecules
5.
Consider the following reaction:
2A
+ B 3C + D
3.0 mol A and 2.0 mol B react to form 4.0 mol C. What is the percent yield of the reaction? A. B. C. D. E.
50% 67% 75% 89% 100%
6. When NH3 is prepared from 28g N2 and excess H2, the theoretical yield of NH3 is 34g. When this reaction is carried out in a given experiment, only 30g is produced. What is the percentage yield?
A. B. C. D. E.
6% 12% 14% 82% 88%
7. The empirical formula for the compound having the formula H2C2O4 is A. B. C. D. E.
COH COH2 C2H2 C2O4H2 CO2H
8. Which of the following has the largest percent by mass of carbon? A. CaCO3 B. CO2 C. CH4 D. NaHCO3 9. A compound is analyzed and found to contain 12.1% carbon, 16.2% oxygen, and 71.7% chlorine (by mass). Calculate the empirical formula of this compound. A. COCl B. COCl2 C. CO2Cl D. CO2Cl2 E. COCl4
10. Calculate the molecular formula of a compound with the empirical formula CH2O and a molar mass of 150g/mol. A. B. C. D. E.
C2H4O2 C3H6O3 C4H8O4 C5H10O5 C6H12O6
11. A certain compound is found to have the percent composition (by mass) of 85.63% C and 14.37% H. The molar mass of the compound was found to be 42.0 g/mol. Calculate the empirical and the molecular formulas. A. B. C. D. E.
C2H3 and C4H6 CH and C3H3 CH2 and C3H6 CH3 and C2H6 C2H6 and C3H9
12. The correct formula for arsenic(III) oxide is A. B. C. D. E.
As3O3 As2O3 As3O2 AsO As3O 13 . Identify the incorrect statement among the following:
A. A mole is that quantity of a substance that contains 6.02x1023 particles of that substance. B. One mole of any substance contains the same number of particles as one mole of any other substance. C. One mole of any substance contains the same number of particles as the number of atoms in exactly 12 grams of carbon-12. D. A mole is a quantity of a substance that has a mass of exactly 12 grams. E. All of the above are correct.
14. In the sum of 54.34 + 45.66, the number of significant figures is A. B. C. D.
2 3 4 5
E. 6
15. The number 0.005802 expressed in scientific notation is A. B. C. D. E.
5.82 x 103 5.802 x 103 5.82 x 10-3 5.802 x 10-3 5802 x 10-6
16. Which of the following is a binary compound? A. O2 B. HCN C. H2SO4 D. H2S E. NaOH
17. Select the correct statement about
43
Ti
A. The nucleus contains 22 protons and 26 neutrons, mass number =48 B. The nucleus contains 22 protons and 21 neutrons, atomic number =22 C. The nucleus contains 21 protons and 22 neutrons, mass number =43. D. The nucleus contains 22 protons and 43 neutrons, atomic number 22 E . None of the above are correct.
18. The sum of the coefficients when the following equation is balanced is BaSO4 + K3PO4 a3 (PO4)2 + A. 4 A. B. C. D.
7 8 9 11
K2SO4
19. The name for HBrO (aq) is A. B. C. D. E.
hydrogen bromous acid bromous acid bromic acid hypobromous acid perbromic acid
20. The reaction AgNO3 (aq) + NaCl (aq) AgCl(s) + NaNO3(aq) is a(n) ------------------ reaction.
A. B. C. D. E.
precipitation acid-base oxidation-reduction none of these single replacement
21. A reaction that involves a transfer of electrons is called a(n) ------- reaction A. B. C. D. E.
precipitation acid –base oxidation-reduction double displacement none of these
IIb) Write a balanced chemical equation for the following: (4) 1. Aqueous hydrochloric acid reacts with solid manganese (IV) oxide to form aqueous manganese (II) chloride, liquid water, and chlorine gas.
2. Liquid nitric acid decomposes to reddish brown nitrogen dioxide gas, liquid water, and oxygen gas. (This is why bottles of nitric acidbecome yellow upon standing).
IIIa) Balance the following chemical equations.(6)
Na2O2(s) + H2O(l) NaOH(aq) + O2(g)
Mg3N2 (s) + H2O (l) NH3(g) + Mg(OH)2 (s)
FeCl3(aq) + KOH (aq) Fe (OH)3 + KCl (aq)
IIIb) Give the name and calculate the molar mass for each of the following:(4) 1.Cr2O3
2. NaOCl
IV)Solve the following: 1.Calculate the theoretical yield of NO and the percentage yield of NO if 49.2g of NO2 yield 8.90 grams of NO in the following reaction:(3 points) 3NO2(g) + H2O (g) 2HNO3(g) + NO(g)
2. Nitrogen gas can be prepared by passing gaseous ammonia over solid copper (II) oxide at high temperatures. The products of the reaction are solid copper and water vapour. How many grams of nitrogen are formed when 18.1g of NH3 are reacted with with 90.4g of CuO? (5 points)
BONUS QUESTION (6 points) Finish the following table. (Use the periodic chart given to you) Nuclear Symbol
# of Protons
34
-----------
S
-----------
23
------------
---------
# of Neutrons
---------------
28
-------------
# of electrons
-------------
------------
Atomic #
------------
------------
13
Mass #
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27
