Question 1

Match the following.

-Mg(s)+ Cu(NO3)2(aq)→ Mg(NO3)2(aq)+ Cu(s)

Accepted Answer

A) acid-base 
B) oxidation-reduction 
C) combustion 
D) gas evolution

Question 2

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction: Fe2O3(s)+ 2Al(s)→ Al2O3(s)+ 2Fe(s)

Accepted Answer

A) 61.03% 
B) 28.65% 
C) 57.30% 
D) 20.02% 
E) 81.93%

Question 3

Define a spectator ion.

Accepted Answer

The answer of Define a spectator ion....

Question 4

Which of the following describes sugar?

Accepted Answer

A) strong electrolyte, weak acid 
B) weak electrolyte, weak acid 
C) strong electrolyte, strong acid 
D) weak electrolyte, strong acid 
E) nonelectrolyte

Question 5

Identify the oxidation state of H in H2(g). Mg(s)+ 2HCl(aq)→ MgCl2(aq)+ H2(g)

Accepted Answer

A) +1 
B) +2 
C) 0 
D) -1 
E) -2

Question 6

Which of the following is a precipitation reaction?

Accepted Answer

A) 2HBr(aq)+ NiS(s)→ NiBr2(aq)+ H2S(g) 
B) NH4I(aq)+ NaOH(aq)→ H2O(l)+ NH3(g)+ NaI(aq) 
C) 2C4H6(g)+ 11O2(g)→ 8CO2(g)+ 6H2O(g) 
D) NO(g)+ H2O(g)→ NH3(g)+ O2(g) 
E) CrBr2(aq)+ Na2CO3(aq)→ CrCO3(s)+ 2NaBr(aq)

Question 7

How many grams of H₃PO₄ are in 265 mL of a 1.50 mol L^-1 solution of H₃PO₄?

Accepted Answer

The answer of How many grams of H₃PO₄ are in...

Question 8

How many millilitres of 0.550 mol L-1 hydriodic acid are needed to react with 15.00 mL of 0.217 mol L-1 CsOH? HI(aq)+ CsOH(aq)→ CsI(aq)+ H2O(l)

Accepted Answer

A) 0.0263 mL 
B) 0.169 mL 
C) 5.92 mL 
D) 38.0 mL

Question 9

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. ________ Al(s)+ ________ I2(s)→ ________ Al2I6(s)

Accepted Answer

A) 0.741 mol 
B) 1.67 mol 
C) 2.22 mol 
D) 3.33 mol

Question 10

Which of the following pairs of aqueous solutions will form a precipitate when mixed?

Accepted Answer

A) HCl + LiOH 
B) Li2S + HCl 
C) K2CO3 + HNO3 
D) MgCl2 + KOH 
E) All of these solution pairs will produce a precipitate.

Question 11

According to the following balanced reaction, how many moles of HNO3 are formed from 8.44 moles of NO2 if there is plenty of water present? 3NO2(g)+ H2O(l)→ 2HNO3(aq)+ NO(g)

Accepted Answer

A) 2.81 moles HNO3 
B) 25.3 moles HNO3 
C) 8.44 moles HNO3 
D) 5.63 moles HNO3 
E) 1.83 moles HNO3

Question 12

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

Accepted Answer

A) 1.50 mol L-1 
B) 1.18 mol L-1 
C) 0.130 mol L-1 
D) 0.768 mol L-1 
E) 2.30 mol L-1

Question 13

Identify the net ionic equation for the reaction (if any)that occurs when aqueous solutions of Na2CO3 and HCl are mixed.

Accepted Answer

A) 2H+(aq)+ CO32-(aq)→ H2CO3(s) 
B) 2Na+(aq)+ CO32-(aq)+ 2H+(aq)+ 2Cl-(aq)→ H2CO3(s)+ 2NaCl(aq) 
C) 2H+(aq)+ CO32-(aq)→ H2O(l)+ CO2(g) 
D) 2Na+(aq)+ CO32-(aq)+ 2H+(aq)+ 2Cl-(aq)→ H2CO3(s)+ 2Na+(aq)+ 2Cl-(aq) 
E) No reaction occurs.

Question 14

What are the required coefficients to properly balance the following chemical reaction?
 Na(s)+ H2O(l)→ H2(g)+ NaOH(aq)

Accepted Answer

A) 1, 2, 2, 1 
B) 2, 2, 1, 1 
C) 2, 1, 1, 1 
D) 2, 1, 2, 1 
E) 2, 2, 1, 2

Question 15

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Accepted Answer

The answer of What is the concentration (M)of a NaCl...

Question 16

Calculate the concentration (M)of sodium ions in a solution made by diluting 40.0 mL of a 0.474 mol L^-1 solution of sodium sulfide to a total volume of 300 mL.

Accepted Answer

The answer of Calculate the concentration (M)of sodium ions in...

Question 17

Identify the balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.

Accepted Answer

A) H2SO4(aq)+ LiOH(aq)→ H2O(l)+ Li2SO4(aq) 
B) H2SO3(aq)+ 2LiOH(aq)→ 2H2O(l)+ Li2SO3(aq) 
C) HSO3(aq)+ LiOH(aq)→ H2O(l)+ LiSO3(aq) 
D) HSO4(aq)+ LiOH(aq)→ H2O(l)+ LiSO4(aq) 
E) H2S(aq)+ 2LiOH(aq)→ 2H2O(l)+ Li2S(aq)

Question 18

How many millilitres of 0.200 mol L-1 FeCl3 are needed to react with an excess of Na2S to produce 1.38 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3Na2S(aq)+ 2FeCl3(aq)→ Fe2S3(s)+ 6NaCl(aq)

Accepted Answer

A) 25.5 mL 
B) 43.1 mL 
C) 51.1 mL 
D) 102 mL

Question 19

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution?

Accepted Answer

A) 0.0101 mol L-1 
B) 0.0404 mol L-1 
C) 0.162 mol L-1 
D) 0.323 mol L-1

Question 20

How many moles of NaCl are required to make 250 mL of a 3.00 mol L-1 solution?

Accepted Answer

A) 750 moles 
B) 0.750 moles 
C) 3 moles 
D) 0.250 moles

Exam 4: Chemical Reactions and Stoichiometry

Match the following. -Mg(s) + Cu(NO₃) ₂(aq) → Mg(NO₃) ₂(aq) + Cu(s)

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe₂O₃ react with excess Al according to the following reaction: Fe₂O₃(s) + 2Al(s) → Al₂O₃(s) + 2Fe(s)

Define a spectator ion.

Which of the following describes sugar?

Identify the oxidation state of H in H₂(g) . Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

Which of the following is a precipitation reaction?

How many grams of H₃PO₄ are in 265 mL of a 1.50 mol L^-1 solution of H₃PO₄?

How many millilitres of 0.550 mol L^-1 hydriodic acid are needed to react with 15.00 mL of 0.217 mol L^-1 CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H₂O(l)

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. Al(s) + I₂(s) → Al₂I₆(s)

Which of the following pairs of aqueous solutions will form a precipitate when mixed?

According to the following balanced reaction, how many moles of HNO₃ are formed from 8.44 moles of NO₂if there is plenty of water present? 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

Identify the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

What are the required coefficients to properly balance the following chemical reaction? Na(s) + H₂O(l) → H₂(g) + NaOH(aq)

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Calculate the concentration (M)of sodium ions in a solution made by diluting 40.0 mL of a 0.474 mol L^-1 solution of sodium sulfide to a total volume of 300 mL.

Identify the balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.

How many millilitres of 0.200 mol L^-1 FeCl₃ are needed to react with an excess of Na₂S to produce 1.38 g of Fe₂S₃ if the percent yield for the reaction is 65.0%? 3Na₂S(aq) + 2FeCl₃(aq) → Fe₂S₃(s) + 6NaCl(aq)

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350. mL of solution?

How many moles of NaCl are required to make 250 mL of a 3.00 mol L^-1 solution?

Exam 4: Chemical Reactions and Stoichiometry

Match the following. -Mg(s) + Cu(NO3) 2(aq) → Mg(NO3) 2(aq) + Cu(s)

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction: Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s)

Define a spectator ion.

Which of the following describes sugar?

Identify the oxidation state of H in H2(g) . Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

Which of the following is a precipitation reaction?

How many grams of H3PO4 are in 265 mL of a 1.50 mol L-1 solution of H3PO4?

How many millilitres of 0.550 mol L-1 hydriodic acid are needed to react with 15.00 mL of 0.217 mol L-1 CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l)

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. ________ Al(s) + ________ I2(s) → ________ Al2I6(s)

Which of the following pairs of aqueous solutions will form a precipitate when mixed?

According to the following balanced reaction, how many moles of HNO3 are formed from 8.44 moles of NO2 if there is plenty of water present? 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

Identify the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.

What are the required coefficients to properly balance the following chemical reaction? Na(s) + H2O(l) → H2(g) + NaOH(aq)

What is the concentration (M)of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Calculate the concentration (M)of sodium ions in a solution made by diluting 40.0 mL of a 0.474 mol L-1 solution of sodium sulfide to a total volume of 300 mL.

Identify the balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.

How many millilitres of 0.200 mol L-1 FeCl3 are needed to react with an excess of Na2S to produce 1.38 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3Na2S(aq) + 2FeCl3(aq) → Fe2S3(s) + 6NaCl(aq)

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution?

How many moles of NaCl are required to make 250 mL of a 3.00 mol L-1 solution?

Match the following. -Mg(s) + Cu(NO₃) ₂(aq) → Mg(NO₃) ₂(aq) + Cu(s)

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe₂O₃ react with excess Al according to the following reaction: Fe₂O₃(s) + 2Al(s) → Al₂O₃(s) + 2Fe(s)

Identify the oxidation state of H in H₂(g) . Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

How many grams of H₃PO₄ are in 265 mL of a 1.50 mol L^-1 solution of H₃PO₄?

How many millilitres of 0.550 mol L^-1 hydriodic acid are needed to react with 15.00 mL of 0.217 mol L^-1 CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H₂O(l)

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. Al(s) + I₂(s) → Al₂I₆(s)

According to the following balanced reaction, how many moles of HNO₃ are formed from 8.44 moles of NO₂if there is plenty of water present? 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

Identify the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

What are the required coefficients to properly balance the following chemical reaction? Na(s) + H₂O(l) → H₂(g) + NaOH(aq)

Calculate the concentration (M)of sodium ions in a solution made by diluting 40.0 mL of a 0.474 mol L^-1 solution of sodium sulfide to a total volume of 300 mL.

How many millilitres of 0.200 mol L^-1 FeCl₃ are needed to react with an excess of Na₂S to produce 1.38 g of Fe₂S₃ if the percent yield for the reaction is 65.0%? 3Na₂S(aq) + 2FeCl₃(aq) → Fe₂S₃(s) + 6NaCl(aq)

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K₃PO₄ in enough water to make 350. mL of solution?

How many moles of NaCl are required to make 250 mL of a 3.00 mol L^-1 solution?