Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g mol-1, HNO3 = 63.02 g mol-1. 3NO2(g)+ H2O(l)→ 2HNO3(aq)+ NO(g)

A) 38.0 g H2O B) 21.7 g H2O C) 43.4 g H2O D) 10.9 g H2O E) 26.5 g H2O A) 38.0 g H2O B) 21.7 g H2O C) 43.4 g H2O D) 10.9 g H2O E) 26.5 g H2O

Determine the oxidation state of Sn in Sn(SO4)2.

A) +2 B) +4 C) +6 D) 0 E) -2 A) +2 B) +4 C) +6 D) 0 E) -2

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ N2(g)→ 2Li3N(s) How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?

A) 0.30 B) 1.8 C) 0.20 D) 0.40 E) 3.6 A) 0.30 B) 1.8 C) 0.20 D) 0.40 E) 3.6

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s)→ 2Na(s)+ 3N2(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

A) 1.77 B) 0.785 C) 76.6 D) 51.1 E) 114.9 A) 1.77 B) 0.785 C) 76.6 D) 51.1 E) 114.9

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O2(g)→ 2MgO(s) How many moles of O2 are consumed when 0.770 mol of magnesium burns?

A) 0.0317 B) 2.60 C) 0.770 D) 1.54 E) 0.385 A) 0.0317 B) 2.60 C) 0.770 D) 1.54 E) 0.385

Determine the reducing agent in the following reaction. 2Li(s)+ Fe(C2H3O2)2(aq)→ 2LiC2H3O2(aq)+ Fe(s)

A) O B) H C) C D) Fe E) Li A) O B) H C) C D) Fe E) Li

A stock solution of HNO3 is prepared and found to contain 13.5 mol L-1 of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?

A) 0.270 mol L-1 B) 1.48 mol L-1 C) 0.675 mol L-1 D) 675 mol L-1 E) 270 mol L-1 A) 0.270 mol L-1 B) 1.48 mol L-1 C) 0.675 mol L-1 D) 675 mol L-1 E) 270 mol L-1

Exam 4: Chemical Reactions and Stoichiometry

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s)+ 2H₂O(l)→ 4KOH(s)+ O₂(g)

(Multiple Choice)

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Question 41

Determine the oxidation state of Mn in KMnO₄.

(Short Answer)

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Question 42

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows: H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g)+ H₂O(l)→ 2HNO₃(aq)+ NO(g)

(Multiple Choice)

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Question 43

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s)→ 2K₂O(s)+ 2N₂(g)+ 5O₂(g)

(Multiple Choice)

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Question 44

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3H₂O → ICl + HIO₃ + 5HCl

(Multiple Choice)

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Question 45

Determine the oxidation state of Sn in Sn(SO₄)₂.

(Multiple Choice)

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Question 46

Aluminum metal reacts with aqueous iron(II)chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

(Multiple Choice)

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Question 47

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: BrO₃^-(aq)+ H⁺(aq)→ Br^-(aq)+ H₂O(l)

(Multiple Choice)

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Question 48

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ N₂(g)→ 2Li₃N(s) How many moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen?

(Multiple Choice)

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Question 49

Determine the theoretical yield of HCl if 60.0 g of BCl₃and 37.5 g of H₂O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl₃ = 117.16 g mol^-1. BCl₃(g)+ 3H₂O(l)→ H₃BO₃(s)+ 3HCl(g)

(Multiple Choice)

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Question 50

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s)→ 2Na(s)+ 3N₂(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

(Multiple Choice)

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Question 51

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq)in the following reaction? BCl₃(g)+ 3H₂O(l)→ 3HCl(aq)+ B(OH)₃(aq)

(Multiple Choice)

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Question 52

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag⁺(aq)+ Cl^-(aq)→ AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.366 mol L^-1 AgNO₃ solution to completely precipitate the silver?

(Multiple Choice)

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Question 53

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O₂(g)→ 2MgO(s) How many moles of O₂ are consumed when 0.770 mol of magnesium burns?

(Multiple Choice)

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Question 54

Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was involved in the reaction?

(Multiple Choice)

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Question 55

Determine the reducing agent in the following reaction. 2Li(s)+ Fe(C₂H₃O₂)₂(aq)→ 2LiC₂H₃O₂(aq)+ Fe(s)

(Multiple Choice)

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Question 56

Which of the following describes NaCl?

(Multiple Choice)

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Question 57

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

(Multiple Choice)

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Question 58

A stock solution of HNO₃ is prepared and found to contain 13.5 mol L^-1 of HNO₃. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?

(Multiple Choice)

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Question 59

Which pair of compounds is soluble in water?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 230

Exam 4: Chemical Reactions and Stoichiometry

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H2O? Assume an excess of KO. 4KO(s)+ 2H2O(l)→ 4KOH(s)+ O2(g)

Determine the oxidation state of Mn in KMnO4.

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g mol-1, HNO3 = 63.02 g mol-1. 3NO2(g)+ H2O(l)→ 2HNO3(aq)+ NO(g)

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g mol-1. 4KNO3(s)→ 2K2O(s)+ 2N2(g)+ 5O2(g)

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3H2O → ICl + HIO3 + 5HCl

Determine the oxidation state of Sn in Sn(SO4)2.

Aluminum metal reacts with aqueous iron(II)chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: Br O3- (aq)+ H+(aq)→ Br-(aq)+ H2O(l)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ N2(g)→ 2Li3N(s) How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g mol-1. BCl3(g)+ 3H2O(l)→ H3BO3(s)+ 3HCl(g)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s)→ 2Na(s)+ 3N2(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq)in the following reaction? BCl3(g)+ 3H2O(l)→ 3HCl(aq)+ B(OH)3(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O2(g)→ 2MgO(s) How many moles of O2 are consumed when 0.770 mol of magnesium burns?

Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was involved in the reaction?

Determine the reducing agent in the following reaction. 2Li(s)+ Fe(C2H3O2)2(aq)→ 2LiC2H3O2(aq)+ Fe(s)

Which of the following describes NaCl?

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

A stock solution of HNO3 is prepared and found to contain 13.5 mol L-1 of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?

Which pair of compounds is soluble in water?

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According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s)+ 2H₂O(l)→ 4KOH(s)+ O₂(g)

Determine the oxidation state of Mn in KMnO₄.

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows: H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g)+ H₂O(l)→ 2HNO₃(aq)+ NO(g)

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s)→ 2K₂O(s)+ 2N₂(g)+ 5O₂(g)

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3H₂O → ICl + HIO₃ + 5HCl

Determine the oxidation state of Sn in Sn(SO₄)₂.

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: BrO₃^-(aq)+ H⁺(aq)→ Br^-(aq)+ H₂O(l)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ N₂(g)→ 2Li₃N(s) How many moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen?

Determine the theoretical yield of HCl if 60.0 g of BCl₃and 37.5 g of H₂O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl₃ = 117.16 g mol^-1. BCl₃(g)+ 3H₂O(l)→ H₃BO₃(s)+ 3HCl(g)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s)→ 2Na(s)+ 3N₂(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq)in the following reaction? BCl₃(g)+ 3H₂O(l)→ 3HCl(aq)+ B(OH)₃(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O₂(g)→ 2MgO(s) How many moles of O₂ are consumed when 0.770 mol of magnesium burns?

Determine the reducing agent in the following reaction. 2Li(s)+ Fe(C₂H₃O₂)₂(aq)→ 2LiC₂H₃O₂(aq)+ Fe(s)

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

A stock solution of HNO₃ is prepared and found to contain 13.5 mol L^-1 of HNO₃. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?