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In an oxidation-reduction reaction, the substance oxidized always


A) experiences a loss of electrons.
B) takes on oxygen atoms.
C) experiences a gain of electrons.
D) becomes a charged species.
E) gives up hydrogen atoms.

F) C) and D)
G) B) and C)

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When 85.0 g of When 85.0 g of are mixed with 160 g of the limiting reactant is A) B) C) D) are mixed with 160 g of When 85.0 g of are mixed with 160 g of the limiting reactant is A) B) C) D) the limiting reactant is When 85.0 g of are mixed with 160 g of the limiting reactant is A) B) C) D)


A) When 85.0 g of are mixed with 160 g of the limiting reactant is A) B) C) D)
B) When 85.0 g of are mixed with 160 g of the limiting reactant is A) B) C) D)
C) When 85.0 g of are mixed with 160 g of the limiting reactant is A) B) C) D)
D) When 85.0 g of are mixed with 160 g of the limiting reactant is A) B) C) D)

E) A) and D)
F) A) and C)

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How many moles of How many moles of are in 15.0 g of A) 0.119 moles B) 0.111 moles C) 0.0861 moles D) 0.172 moles E) 2.61 x 10<sup>3</sup> moles are in 15.0 g of How many moles of are in 15.0 g of A) 0.119 moles B) 0.111 moles C) 0.0861 moles D) 0.172 moles E) 2.61 x 10<sup>3</sup> moles


A) 0.119 moles
B) 0.111 moles
C) 0.0861 moles
D) 0.172 moles
E) 2.61 x 103 moles

F) C) and E)
G) A) and B)

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Barium chloride and sodium sulfate react according to the following equation. Barium chloride and sodium sulfate react according to the following equation. Answer the question(s) that follow about this reaction. -How many moles of barium sulfate are produced from 0.100 mole of barium chloride? A) 0.100 mole B) 1.00 mole C) 2.00 moles D) 0.0100 mole E) 0.200 mole Answer the question(s) that follow about this reaction. -How many moles of barium sulfate are produced from 0.100 mole of barium chloride?


A) 0.100 mole
B) 1.00 mole
C) 2.00 moles
D) 0.0100 mole
E) 0.200 mole

F) A) and B)
G) None of the above

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For the question(s) that follow, consider the following equation. For the question(s) that follow, consider the following equation. -When 2 moles of are allowed to react, how many moles of also react? A) 6 moles B) 4 moles C) 1 mole D) 12 moles E) 8 moles -When 2 moles of For the question(s) that follow, consider the following equation. -When 2 moles of are allowed to react, how many moles of also react? A) 6 moles B) 4 moles C) 1 mole D) 12 moles E) 8 moles are allowed to react, how many moles of For the question(s) that follow, consider the following equation. -When 2 moles of are allowed to react, how many moles of also react? A) 6 moles B) 4 moles C) 1 mole D) 12 moles E) 8 moles also react?


A) 6 moles
B) 4 moles
C) 1 mole
D) 12 moles
E) 8 moles

F) A) and E)
G) A) and B)

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1.25 moles of 1.25 moles of have a mass of A) 279 g. B) 299 g. C) 239 g. D) 191 g. E) 178 g. have a mass of


A) 279 g.
B) 299 g.
C) 239 g.
D) 191 g.
E) 178 g.

F) All of the above
G) C) and E)

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When 60.0 g of When 60.0 g of reacts with excess the actual yield of is 112 g. What is the percent yield? A) 67.9 % B) 46.4 % C) 187 % D) 53.6 % reacts with excess When 60.0 g of reacts with excess the actual yield of is 112 g. What is the percent yield? A) 67.9 % B) 46.4 % C) 187 % D) 53.6 % the actual yield of When 60.0 g of reacts with excess the actual yield of is 112 g. What is the percent yield? A) 67.9 % B) 46.4 % C) 187 % D) 53.6 % is 112 g. What is the percent yield? When 60.0 g of reacts with excess the actual yield of is 112 g. What is the percent yield? A) 67.9 % B) 46.4 % C) 187 % D) 53.6 %


A) 67.9 %
B) 46.4 %
C) 187 %
D) 53.6 %

E) B) and C)
F) A) and B)

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What is the molar mass of sodium phosphate, What is the molar mass of sodium phosphate, A) 308 g B) 119 g C) 164 g D) 226 g E) 354 g


A) 308 g
B) 119 g
C) 164 g
D) 226 g
E) 354 g

F) C) and D)
G) A) and C)

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Find the mass of Find the mass of that is produced when 10.0 grams of react with 10.0 g of HCl according to the following equation. A) 10.0 g B) 6.10 g C) 16.2 g D) 12.2 g E) 20.0 g that is produced when 10.0 grams of Find the mass of that is produced when 10.0 grams of react with 10.0 g of HCl according to the following equation. A) 10.0 g B) 6.10 g C) 16.2 g D) 12.2 g E) 20.0 g react with 10.0 g of HCl according to the following equation. Find the mass of that is produced when 10.0 grams of react with 10.0 g of HCl according to the following equation. A) 10.0 g B) 6.10 g C) 16.2 g D) 12.2 g E) 20.0 g


A) 10.0 g
B) 6.10 g
C) 16.2 g
D) 12.2 g
E) 20.0 g

F) A) and B)
G) B) and C)

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What is the classification for this balanced reaction? What is the classification for this balanced reaction? A) double replacement B) decomposition C) combination D) combustion E) single replacement


A) double replacement
B) decomposition
C) combination
D) combustion
E) single replacement

F) A) and B)
G) B) and D)

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For the question(s) that follow, consider the following equation. For the question(s) that follow, consider the following equation. -How many grams of are needed to produce 150 g of A) 23 g B) 18 g C) 46 g D) 93 g E) 130 g -How many grams of For the question(s) that follow, consider the following equation. -How many grams of are needed to produce 150 g of A) 23 g B) 18 g C) 46 g D) 93 g E) 130 g are needed to produce 150 g of For the question(s) that follow, consider the following equation. -How many grams of are needed to produce 150 g of A) 23 g B) 18 g C) 46 g D) 93 g E) 130 g


A) 23 g
B) 18 g
C) 46 g
D) 93 g
E) 130 g

F) C) and E)
G) B) and C)

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What is the molar mass of NaBr?

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How many atoms of neon are present in 1.30 moles of neon?


A) How many atoms of neon are present in 1.30 moles of neon? A) B) C) D) E)
B) How many atoms of neon are present in 1.30 moles of neon? A) B) C) D) E)
C) How many atoms of neon are present in 1.30 moles of neon? A) B) C) D) E)
D) How many atoms of neon are present in 1.30 moles of neon? A) B) C) D) E)
E) How many atoms of neon are present in 1.30 moles of neon? A) B) C) D) E)

F) None of the above
G) A) and D)

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4.00 moles of sodium have a mass of


A) 44.0 g.
B) 23.0 g.
C) 11.0 g.
D) 4.60 g.
E) 92.0 g.

F) B) and E)
G) C) and D)

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For the reaction: For the reaction: how many kcal are needed to react A) 274 kcal B) 190 kcal C) 760. kcal D) 137 kcal E) 380 kcal how many kcal are needed to react For the reaction: how many kcal are needed to react A) 274 kcal B) 190 kcal C) 760. kcal D) 137 kcal E) 380 kcal


A) 274 kcal
B) 190 kcal
C) 760. kcal
D) 137 kcal
E) 380 kcal

F) C) and E)
G) B) and E)

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In the following reaction, when the equation is correctly balanced, what is the correct coefficient for aluminum chloride? In the following reaction, when the equation is correctly balanced, what is the correct coefficient for aluminum chloride? A) 1 B) 2 C) 3 D) 4 E) 5


A) 1
B) 2
C) 3
D) 4
E) 5

F) B) and C)
G) B) and D)

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