Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3 Mg + N2 → Mg3N2 In a particular experiment, a 8.33-g sample of N2 reacts completely. The mass of Mg consumed is ________ g.

A) 7.23 B) 21.7 C) 28.9 D) 0.92 E) 13.9 A) 7.23 B) 21.7 C) 28.9 D) 0.92 E) 13.9

There are ________ atoms of oxygen in 300 molecules of CH3CO2H.

A) 300 B) 600 C) 150 D) 3.6 × 1026 E) 1.0 × 10-22 A) 300 B) 600 C) 150 D) 3.6 × 1026 E) 1.0 × 10-22

Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of methanol in the balanced equation?

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

Combustion of a 0.9827-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of H2O. What is the empirical formula of the compound?

A) C2H5O B) C4H10O2 C) C4H11O2 D) C4H10O E) C2H5O2 A) C2H5O B) C4H10O2 C) C4H11O2 D) C4H10O E) C2H5O2

Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of oxygen in the balanced equation?

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

Calcium carbide (CaC2)reacts with water to produce acetylene (C2H2): CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g) Production of 6.5 g of C2H2 requires consumption of ________ g of H2O.

A) 2.3 B) 4.5 C) 9.0 D) 480 E) 0.048 A) 2.3 B) 4.5 C) 9.0 D) 480 E) 0.048

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O2 (g) → 2MgO (s) When 5.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.

A) 5.50 B) 9.12 C) 0.226 D) 4.56 E) 18.2 A) 5.50 B) 9.12 C) 0.226 D) 4.56 E) 18.2

The mass % of H in methane (CH4)is ________.

A) 25.13 B) 4.032 C) 74.87 D) 92.26 E) 7.743 A) 25.13 B) 4.032 C) 74.87 D) 92.26 E) 7.743

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 28.0 g of nitrogen?

A) 1.50 B) 0.666 C) 65.0 D) 43.3 E) 97.5 A) 1.50 B) 0.666 C) 65.0 D) 43.3 E) 97.5

The combustion of propane (C3H8)produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) The reaction of 2.5 mol of O2 will produce ________ mol of H2O.

A) 4.0 B) 3.0 C) 2.5 D) 2.0 E) 1.0 A) 4.0 B) 3.0 C) 2.5 D) 2.0 E) 1.0

Exam 3: Stoichiometry: Calculations With Chemical Formulas and Equations

Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3 Mg + N₂ → Mg₃N₂ In a particular experiment, a 8.33-g sample of N₂ reacts completely. The mass of Mg consumed is ________ g.

(Multiple Choice)

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Question 101

A compound contains 38.7% K, 13.9% N, and 47.4% O by mass. What is the empirical formula of the compound?

(Multiple Choice)

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Question 102

When the following equation is balanced, the coefficient of dinitrogen pentoxide is ________. N₂O₅ (g) + H₂O (l) → HNO₃ (aq)

(Multiple Choice)

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Question 103

There are ________ atoms of oxygen in 300 molecules of CH₃CO₂H.

(Multiple Choice)

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Question 104

Write the balanced equation for the reaction that occurs when methanol, CH₃OH (l), is burned in air. What is the coefficient of methanol in the balanced equation?

(Multiple Choice)

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Question 105

Combustion of a 0.9827-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of CO₂ and 1.070 g of H₂O. What is the empirical formula of the compound?

(Multiple Choice)

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Question 106

What is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by mass?

(Multiple Choice)

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Question 107

If 588 grams of FeS₂ is allowed to react with 352 grams of O₂ according to the following equation, how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

(Short Answer)

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Question 108

Calculate the percentage by mass of lead in PbCO₃.

(Multiple Choice)

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Question 109

Write the balanced equation for the reaction that occurs when methanol, CH₃OH (l), is burned in air. What is the coefficient of oxygen in the balanced equation?

(Multiple Choice)

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Question 110

Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂): CaC₂ (s) + 2H₂O (g) → Ca(OH)₂ (s) + C₂H₂ (g) Production of 6.5 g of C₂H₂ requires consumption of ________ g of H₂O.

(Multiple Choice)

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Question 111

What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?

(Multiple Choice)

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Question 112

Of the reactions below, which one is not a combination reaction?

(Multiple Choice)

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Question 113

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O₂ (g) → 2MgO (s) When 5.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.

(Multiple Choice)

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Question 114

Calculate the percentage by mass of chlorine in PtCl₂(NH₃)₂.

(Multiple Choice)

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Question 115

The mass % of H in methane (CH₄)is ________.

(Multiple Choice)

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Question 116

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 28.0 g of nitrogen?

(Multiple Choice)

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Question 117

There are ________ mol of carbon atoms in 5 mol of dimethylsulfoxide (C₂H₆SO).

(Multiple Choice)

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Question 118

Determine the mass percent (to the hundredths place)of C in sodium bicarbonate (NaHCO₃).

(Short Answer)

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Question 119

The combustion of propane (C₃H₈)produces CO₂ and H₂O: C₃H₈ (g) + 5O₂ (g) → 3CO₂ (g) + 4H₂O (g) The reaction of 2.5 mol of O₂ will produce ________ mol of H₂O.

(Multiple Choice)

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Question 120

Showing 101 - 120 of 178

Exam 3: Stoichiometry: Calculations With Chemical Formulas and Equations

Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3 Mg + N2 → Mg3N2 In a particular experiment, a 8.33-g sample of N2 reacts completely. The mass of Mg consumed is ________ g.

A compound contains 38.7% K, 13.9% N, and 47.4% O by mass. What is the empirical formula of the compound?

When the following equation is balanced, the coefficient of dinitrogen pentoxide is ________. N2O5 (g) + H2O (l) → HNO3 (aq)

There are ________ atoms of oxygen in 300 molecules of CH3CO2H.

Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of methanol in the balanced equation?

Combustion of a 0.9827-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of H2O. What is the empirical formula of the compound?

What is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by mass?

If 588 grams of FeS2 is allowed to react with 352 grams of O2 according to the following equation, how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

Calculate the percentage by mass of lead in PbCO3.

Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of oxygen in the balanced equation?

Calcium carbide (CaC2)reacts with water to produce acetylene (C2H2): CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g) Production of 6.5 g of C2H2 requires consumption of ________ g of H2O.

What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?

Of the reactions below, which one is not a combination reaction?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O2 (g) → 2MgO (s) When 5.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.

Calculate the percentage by mass of chlorine in PtCl2(NH3)2.

The mass % of H in methane (CH4)is ________.

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 28.0 g of nitrogen?

There are ________ mol of carbon atoms in 5 mol of dimethylsulfoxide (C2H6SO).

Determine the mass percent (to the hundredths place)of C in sodium bicarbonate (NaHCO3).

The combustion of propane (C3H8)produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) The reaction of 2.5 mol of O2 will produce ________ mol of H2O.

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Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3 Mg + N₂ → Mg₃N₂ In a particular experiment, a 8.33-g sample of N₂ reacts completely. The mass of Mg consumed is ________ g.

When the following equation is balanced, the coefficient of dinitrogen pentoxide is ________. N₂O₅ (g) + H₂O (l) → HNO₃ (aq)

There are ________ atoms of oxygen in 300 molecules of CH₃CO₂H.

Write the balanced equation for the reaction that occurs when methanol, CH₃OH (l), is burned in air. What is the coefficient of methanol in the balanced equation?

Combustion of a 0.9827-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of CO₂ and 1.070 g of H₂O. What is the empirical formula of the compound?

If 588 grams of FeS₂ is allowed to react with 352 grams of O₂ according to the following equation, how many grams of Fe₂O₃ are produced? FeS₂ + O₂ → Fe₂O₃ + SO₂

Calculate the percentage by mass of lead in PbCO₃.

Write the balanced equation for the reaction that occurs when methanol, CH₃OH (l), is burned in air. What is the coefficient of oxygen in the balanced equation?

Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂): CaC₂ (s) + 2H₂O (g) → Ca(OH)₂ (s) + C₂H₂ (g) Production of 6.5 g of C₂H₂ requires consumption of ________ g of H₂O.

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O₂ (g) → 2MgO (s) When 5.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.

Calculate the percentage by mass of chlorine in PtCl₂(NH₃)₂.

The mass % of H in methane (CH₄)is ________.

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 28.0 g of nitrogen?

There are ________ mol of carbon atoms in 5 mol of dimethylsulfoxide (C₂H₆SO).

Determine the mass percent (to the hundredths place)of C in sodium bicarbonate (NaHCO₃).

The combustion of propane (C₃H₈)produces CO₂ and H₂O: C₃H₈ (g) + 5O₂ (g) → 3CO₂ (g) + 4H₂O (g) The reaction of 2.5 mol of O₂ will produce ________ mol of H₂O.