Gram Formula Mass
The formula mass of a compound is the
1)sum of the atomic masses of its atoms
2)sum of the atomic numbers of its atoms
3)product of the atomic masses of its atoms
4)products of the atomic numbers of its atoms
The formula mass of a compound is the
1)sum of the atomic masses of its atoms
2)sum of the atomic numbers of its atoms
3)product of the atomic masses of its atoms
4)products of the atomic numbers of its atoms
6. Which quantity can be calculated for a solid compound, given only the formula of the compound and the Periodic Table of the Elements?
A) the density of the compound
B) the heat of fusion of the compound
C) the melting point of each element in the compound
D) the percent composition by mass of each element in the compound
6. Which quantity can be calculated for a solid compound, given only the formula of the compound and the Periodic Table of the Elements?
A) the density of the compound
B) the heat of fusion of the compound
C) the melting point of each element in the compound
D) the percent composition by mass of each element in the compound
11. Which sample contains a mole of atoms?
A) 23 g Na B) 24 g C C) 42 g Kr D) 78 g K
11. Which sample contains a mole of atoms?
A) 23 g Na B) 24 g C C) 42 g Kr D) 78 g K
16. The coefficients in a balanced chemical equation represent
A) the mass ratios of the substances in the reaction
B) the mole ratios of the substances in the reaction
C) the total number of electrons in the reaction
D) the total number of elements in the reaction
16. The coefficients in a balanced chemical equation represent
A) the mass ratios of the substances in the reaction
B) the mole ratios of the substances in the reaction
C) the total number of electrons in the reaction
D) the total number of elements in the reaction
21. Which type of reaction occurs when a compound is separated into its elements?
A) synthesis
B) decomposition
C) single replacement
D) double replacement
21. Which type of reaction occurs when a compound is separated into its elements?
A) synthesis
B) decomposition
C) single replacement
D) double replacement
2. A 1.0-mole sample of krypton gas has a mass of
A) 19 g B) 36 g C) 39 g D) 84 g
2. A 1.0-mole sample of krypton gas has a mass of
A) 19 g B) 36 g C) 39 g D) 84 g
7. Which compound has the smallest percent composition by mass of chlorine?
A) HCl B) KCl C) LiCl D) NaCl
7. Which compound has the smallest percent composition by mass of chlorine?
A) HCl B) KCl C) LiCl D) NaCl
12. A sample of a compound contains 65.4 grams of zinc, 12.0 grams of carbon, and 48.0 grams of oxygen. What is the mole ratio of zinc to carbon to oxygen in this compound?
A) 1:1:2 B) 1:1:3 C) 1:4:6 D) 5:1:4
12. A sample of a compound contains 65.4 grams of zinc, 12.0 grams of carbon, and 48.0 grams of oxygen. What is the mole ratio of zinc to carbon to oxygen in this compound?
A) 1:1:2 B) 1:1:3 C) 1:4:6 D) 5:1:4
17. Given the incomplete equation representing a reaction:
2C6H14 + ____O2 ------ 12CO2 + 14H2O
What is the coefficient of O2 when the equation is completely balanced using the smallest whole-number coefficients?
A) 13 B) 14 C) 19 D) 26
17. Given the incomplete equation representing a reaction:
2C6H14 + ____O2 ------ 12CO2 + 14H2O
What is the coefficient of O2 when the equation is completely balanced using the smallest whole-number coefficients?
A) 13 B) 14 C) 19 D) 26
22. Which equation represents a single replacement reaction?
A) 2Al(s) + 3Cl2(g) ---- 2AlCl3(s)
B) 2Al(s) + 6HCl(aq) ---- 2AlCl3(aq) + 3H2(g)
C) 2AlCl3(s) ---- 2Al(s) + 3Cl2(g)
D) AlCl3(aq) + 3KOH(aq) ---- Al(OH)3(s) +
3KCl(aq)
22. Which equation represents a single replacement reaction?
A) 2Al(s) + 3Cl2(g) ---- 2AlCl3(s)
B) 2Al(s) + 6HCl(aq) ---- 2AlCl3(aq) + 3H2(g)
C) 2AlCl3(s) ---- 2Al(s) + 3Cl2(g)
D) AlCl3(aq) + 3KOH(aq) ---- Al(OH)3(s) +
3KCl(aq)
3. Which substance has the greatest molecular mass?
A) H2O2 B) NO C) CF2 D) I2
3. Which substance has the greatest molecular mass?
A) H2O2 B) NO C) CF2 D) I2
8. What is the percent composition by mass of nitrogen in (NH4)2CO3 (gram-formula mass = 96.0 g/mol)?
A) 14.6% B) 29.2% C) 58.4% D) 87.5%
8. What is the percent composition by mass of nitrogen in (NH4)2CO3 (gram-formula mass = 96.0 g/mol)?
A) 14.6% B) 29.2% C) 58.4% D) 87.5%
13. What is the mass in grams of 2.0 moles of NO2?
A) 92 B) 60. C) 46 D) 30.
13. What is the mass in grams of 2.0 moles of NO2?
A) 92 B) 60. C) 46 D) 30.
18. Which chemical equation is correctly balanced?
A) H2(g) + O2(g) --- H2O(g)
B) N2(g) + H2(g) --- NH3(g)
C) 2NaCl(s) --- Na(s) + Cl2(g)
D) 2KCl(s) --- 2K(s) + Cl2(g)
18. Which chemical equation is correctly balanced?
A) H2(g) + O2(g) --- H2O(g)
B) N2(g) + H2(g) --- NH3(g)
C) 2NaCl(s) --- Na(s) + Cl2(g)
D) 2KCl(s) --- 2K(s) + Cl2(g)
23. Given the balanced equation:
AgNO3(aq) + NaCl(aq) --- NaNO3 (aq) + AgCl(s)
This reaction is classified as
A) synthesis
B) decomposition
C) single replacement
D) double replacement
23. Given the balanced equation:
AgNO3(aq) + NaCl(aq) --- NaNO3 (aq) + AgCl(s)
This reaction is classified as
A) synthesis
B) decomposition
C) single replacement
D) double replacement
4. What is the gram molecular mass of 1 mole of C3H5(OH)3?
A) 48 g B) 58 g C) 74 g D) 92 g
4. What is the gram molecular mass of 1 mole of C3H5(OH)3?
A) 48 g B) 58 g C) 74 g D) 92 g
9. The percent by mass of water in the hydrate Na2SO4•10H2O is closest to
A) 18% B) 44% C) 56% D) 76%
9. The percent by mass of water in the hydrate Na2SO4•10H2O is closest to
A) 18% B) 44% C) 56% D) 76%
14. Given the balanced equation representing a reaction:
2NO + O2 ---- 2NO2 + energy
The mole ratio of NO to NO2 is
A) 1 to 1 B) 2 to 1 C) 3 to 2 D) 5 to 2
14. Given the balanced equation representing a reaction:
2NO + O2 ---- 2NO2 + energy
The mole ratio of NO to NO2 is
A) 1 to 1 B) 2 to 1 C) 3 to 2 D) 5 to 2
19. Given the incomplete equation for the combustion of ethane:
2C2H6+ 7O2 ---- 4CO2 + 6 ___
What is the formula of the missing product?
A) CH3OH B) HCOOH C) H2O D) H2O2
19. Given the incomplete equation for the combustion of ethane:
2C2H6+ 7O2 ---- 4CO2 + 6 ___
What is the formula of the missing product?
A) CH3OH B) HCOOH C) H2O D) H2O2
24. Based on Table F, which compound is least soluble in water?
A) AlPO4 B) Li2SO4C) Ca(OH)2 D) AgC2H3O2
24. Based on Table F, which compound is least soluble in water?
A) AlPO4 B) Li2SO4C) Ca(OH)2 D) AgC2H3O2
5. What is the gram formula mass of Na2CO3 • 10H2O?
A) 106 g B) 142 g C) 266 g D) 286 g
5. What is the gram formula mass of Na2CO3 • 10H2O?
A) 106 g B) 142 g C) 266 g D) 286 g
10. A student obtained the following data to determine the percent by mass of water in a hydrate.
Mass of crucible + cover - 11.70 g
Mass of crucible + cover + hydrated salt before heating - 14.90 g
Mass of crucible + cover + anhydrous salt after heating - 14.53 g
What is the approximate percent by mass of the water in the hydrated salt?
A) 2.5% B) 12% C) 88% D) 98%
10. A student obtained the following data to determine the percent by mass of water in a hydrate.
Mass of crucible + cover - 11.70 g
Mass of crucible + cover + hydrated salt before heating - 14.90 g
Mass of crucible + cover + anhydrous salt after heating - 14.53 g
What is the approximate percent by mass of the water in the hydrated salt?
A) 2.5% B) 12% C) 88% D) 98%
15. Given the balanced equation representing a reaction: C3H8(g) +5O2(g) 3CO2(g) + 4H2O(g)
What is the total number of moles of O2(g) required for the complete combustion of 1.5 moles of C3H8(g)?
A) .30 mol B) 1.5 mol C) 4.5 mol D) 7.5 mol
15. Given the balanced equation representing a reaction: C3H8(g) +5O2(g) 3CO2(g) + 4H2O(g)
What is the total number of moles of O2(g) required for the complete combustion of 1.5 moles of C3H8(g)?
A) .30 mol B) 1.5 mol C) 4.5 mol D) 7.5 mol
20. Given the unbalanced equation:
__Mg(ClO3)2 ---- __MgCl2 + __O2
What is the coefficient of O2 when the equation is balanced correctly using the smallest whole number coefficients?
A) 1 B) 2 C) 3 D) 4
20. Given the unbalanced equation:
__Mg(ClO3)2 ---- __MgCl2 + __O2
What is the coefficient of O2 when the equation is balanced correctly using the smallest whole number coefficients?
A) 1 B) 2 C) 3 D) 4
25. When PbI2(s) is added to Na2CO3(aq), a white precipitate is formed. According to Reference Table F, the white precipitate most likely is
A) KNO3 B) PbCO3C) NaI D) Na2CO3
25. When PbI2(s) is added to Na2CO3(aq), a white precipitate is formed. According to Reference Table F, the white precipitate most likely is
A) KNO3 B) PbCO3C) NaI D) Na2CO3