When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO2 and 1.01 g of H2O were produced. What is the empirical formula of the compound

A) C2H6O B) C3H6O C) C3H8O D) C2H6O3 E) None of the above A) C2H6O B) C3H6O C) C3H8O D) C2H6O3 E) None of the above

One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na 3(CO3)(HCO3)$\times$2H2O, as shown in the following reaction: 2Na3(CO3)(HCO3)$\rarr$2H2O(s) $\rarr$3Na2CO3(s) + CO2(g) + 5H2O(g) When 15 metric tons (1 * 103 kg) of trona is decomposed, 11 metric tons of Na2CO3 is recovered. What is the percent yield of this reaction? (1 metric ton = 103 kg)

A) 13% B) 42% C) 65% D) 73% E) 95% A) 13% B) 42% C) 65% D) 73% E) 95%

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC2(s) + H2O(l) $\rarr$ HCCH(g) + CaO(s) How many grams of CaC2 would be required to generate 0.20 moles of HCCH(g)

A) 11 g of CaC2 would be required B) 13 g of CaC2 would be required C) 15 g of CaC2 would be required D) 17 g of CaC2 would be required E) None of the above are correct A) 11 g of CaC2 would be required B) 13 g of CaC2 would be required C) 15 g of CaC2 would be required D) 17 g of CaC2 would be required E) None of the above are correct

How many moles of C are in 1.22 moles of C6H12O6

A) 7.32 moles C B) 87.9 moles C C) 1.22 moles C D) 14.7 moles C E) 2.44 moles C A) 7.32 moles C B) 87.9 moles C C) 1.22 moles C D) 14.7 moles C E) 2.44 moles C

A compound with an empirical formula of C2H4Br has a molar mass of 215.90 g/mol. What is the molecular formula

A) C4H8Br2 B) C2H4Br C) CHBr D) C6H12Br3 E) C4H8Br A) C4H8Br2 B) C2H4Br C) CHBr D) C6H12Br3 E) C4H8Br

Calculate the molar mass of (NH4)2SO4.

A) 114.11 g/mol B) 228.22 g/mol C) 118.14 g/mol D) 63.09 g/mol E) 132.15 g/mol A) 114.11 g/mol B) 228.22 g/mol C) 118.14 g/mol D) 63.09 g/mol E) 132.15 g/mol

What is the mass of 3.00 moles of ethanol, C2H6O

A) 4.99 * 10-24 g B) 138 g C) 6.52 * 10-2 g D) 50.0 g E) 1.81 * 1024 g A) 4.99 * 10-24 g B) 138 g C) 6.52 * 10-2 g D) 50.0 g E) 1.81 * 1024 g

Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 $\rarr$ 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react

A) 1.30 mol B) 1.57 mol C) 1.87 mol D) 3.53 mol E) None of these. A) 1.30 mol B) 1.57 mol C) 1.87 mol D) 3.53 mol E) None of these.

What is the mass of 3.50 x 1024 Ti atoms

A) 47.9 amu B) 47.9 g C) 5.81 g D) 278 g E) 5.81 amu A) 47.9 amu B) 47.9 g C) 5.81 g D) 278 g E) 5.81 amu

Exam 3: Mass Relationships in Chemical Reactions

When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced. What is the empirical formula of the compound

(Multiple Choice)

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Question 121

One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na ₃(CO₃)(HCO₃) $\times$ 2H₂O, as shown in the following reaction: 2Na₃(CO₃)(HCO₃) $\rarr$ 2H₂O(s) $\rarr$ 3Na₂CO₃(s) + CO₂(g) + 5H₂O(g) When 15 metric tons (1 * 10³ kg) of trona is decomposed, 11 metric tons of Na₂CO₃ is recovered. What is the percent yield of this reaction? (1 metric ton = 10³ kg)

(Multiple Choice)

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Question 122

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC₂(s) + H₂O(l) $\rarr$ HCCH(g) + CaO(s) How many grams of CaC₂ would be required to generate 0.20 moles of HCCH(g)

(Multiple Choice)

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Question 123

How many moles of C are in 1.22 moles of C₆H₁₂O₆

(Multiple Choice)

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Question 124

A compound with an empirical formula of C₂H₄Br has a molar mass of 215.90 g/mol. What is the molecular formula

(Multiple Choice)

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Question 125

Phosgene, a poisonous gas used during WWI, is composed of 12.1% C, 16.2% O, and 71.1% Cl. What is the empirical formula of phosgene

(Multiple Choice)

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Question 126

Calculate the molar mass of (NH₄)₂SO₄.

(Multiple Choice)

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Question 127

A compound with a percent composition by mass of 87.5% N and 12.5% H was recently discovered. What is the empirical formula for this compound

(Multiple Choice)

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Question 128

Determine the number of moles of aluminum in 96.7 g of Al.

(Multiple Choice)

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Question 129

What is the mass of 3.00 moles of ethanol, C₂H₆O

(Multiple Choice)

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Question 130

Oxidation of a hydrocarbon gave a product composed of carbon, hydrogen, and oxygen. The product that was purified and sent off for elemental analysis giving the following mass percents: 68.85% C and 4.95% H. Determine the empirical formula of this compound.

(Multiple Choice)

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Question 131

What percent by mass of oxygen is present in carbon monoxide, CO

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Question 132

Boron obtained from borax deposits in Death Valley consists of two isotopes. They are boron-10 and boron-11 with atomic masses of 10.013 amu and 11.009 amu, respectively. The atomic mass of boron is 10.81 amu (see periodic table). Which isotope of boron is more abundant, boron-10 or boron-11

(Multiple Choice)

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Question 133

Calculate the mass of 4.50 moles of chlorine gas, Cl₂.

(Multiple Choice)

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Question 134

Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH₃ + 5O₂ $\rarr$ 4NO + 6H₂O What is the theoretical yield of water, in moles, when 40.0 g NH₃ and 50.0 g O₂ are mixed and allowed to react

(Multiple Choice)

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Question 135

What is the theoretical yield of PI₃ if 48.0 g of I₂ are reacted with an excess of phosphorus according to the following chemical equation? 2P(s) + 3I₂(s) $\rarr$ 2PI₃(s)

(Multiple Choice)

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Question 136

Hydrogen gas is reacted with nitrogen gas to form ammonia gas. Write the balanced reaction (omit state symbols (s), (l), (g), (aq), etc.).

(Multiple Choice)

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Question 137

What is the mass of 3.50 x 10²⁴ Ti atoms

(Multiple Choice)

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Question 138

Liquid heptane, C₇H₁₆, burns in oxygen gas to yield carbon dioxide and water. What mass of water is produced when 15.0 mL of heptane burns completely (density of heptane = 0.6838 g/mL)

(Multiple Choice)

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Question 139

A mass spectrometer works by ionizing atoms or molecules, and then accelerating them through oppositely charged plates. The mass is obtained by

(Multiple Choice)

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Question 140

Showing 121 - 140 of 194

Exam 3: Mass Relationships in Chemical Reactions

When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO2 and 1.01 g of H2O were produced. What is the empirical formula of the compound

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC2(s) + H2O(l) →\rarr→ HCCH(g) + CaO(s) How many grams of CaC2 would be required to generate 0.20 moles of HCCH(g)

How many moles of C are in 1.22 moles of C6H12O6

A compound with an empirical formula of C2H4Br has a molar mass of 215.90 g/mol. What is the molecular formula

Phosgene, a poisonous gas used during WWI, is composed of 12.1% C, 16.2% O, and 71.1% Cl. What is the empirical formula of phosgene

Calculate the molar mass of (NH4)2SO4.

A compound with a percent composition by mass of 87.5% N and 12.5% H was recently discovered. What is the empirical formula for this compound

Determine the number of moles of aluminum in 96.7 g of Al.

What is the mass of 3.00 moles of ethanol, C2H6O

Oxidation of a hydrocarbon gave a product composed of carbon, hydrogen, and oxygen. The product that was purified and sent off for elemental analysis giving the following mass percents: 68.85% C and 4.95% H. Determine the empirical formula of this compound.

What percent by mass of oxygen is present in carbon monoxide, CO

Boron obtained from borax deposits in Death Valley consists of two isotopes. They are boron-10 and boron-11 with atomic masses of 10.013 amu and 11.009 amu, respectively. The atomic mass of boron is 10.81 amu (see periodic table). Which isotope of boron is more abundant, boron-10 or boron-11

Calculate the mass of 4.50 moles of chlorine gas, Cl2.

Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 →\rarr→ 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react

What is the theoretical yield of PI3 if 48.0 g of I2 are reacted with an excess of phosphorus according to the following chemical equation? 2P(s) + 3I2(s) →\rarr→ 2PI3(s)

Hydrogen gas is reacted with nitrogen gas to form ammonia gas. Write the balanced reaction (omit state symbols (s), (l), (g), (aq), etc.).

What is the mass of 3.50 x 1024 Ti atoms

Liquid heptane, C7H16, burns in oxygen gas to yield carbon dioxide and water. What mass of water is produced when 15.0 mL of heptane burns completely (density of heptane = 0.6838 g/mL)

A mass spectrometer works by ionizing atoms or molecules, and then accelerating them through oppositely charged plates. The mass is obtained by

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When a 0.860 g sample of an organic compound containing C, H, and O was burned completely in oxygen, 1.64 g of CO₂ and 1.01 g of H₂O were produced. What is the empirical formula of the compound

Acetylene gas, HCCH(g), can be generated in the laboratory by adding calcium carbide to excess water, as shown in the following reaction CaC₂(s) + H₂O(l) $\rarr$ HCCH(g) + CaO(s) How many grams of CaC₂ would be required to generate 0.20 moles of HCCH(g)

How many moles of C are in 1.22 moles of C₆H₁₂O₆

A compound with an empirical formula of C₂H₄Br has a molar mass of 215.90 g/mol. What is the molecular formula

Calculate the molar mass of (NH₄)₂SO₄.

What is the mass of 3.00 moles of ethanol, C₂H₆O

Calculate the mass of 4.50 moles of chlorine gas, Cl₂.

Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH₃ + 5O₂ $\rarr$ 4NO + 6H₂O What is the theoretical yield of water, in moles, when 40.0 g NH₃ and 50.0 g O₂ are mixed and allowed to react

What is the theoretical yield of PI₃ if 48.0 g of I₂ are reacted with an excess of phosphorus according to the following chemical equation? 2P(s) + 3I₂(s) $\rarr$ 2PI₃(s)

What is the mass of 3.50 x 10²⁴ Ti atoms

Liquid heptane, C₇H₁₆, burns in oxygen gas to yield carbon dioxide and water. What mass of water is produced when 15.0 mL of heptane burns completely (density of heptane = 0.6838 g/mL)