How many O atoms are in 4.39 g of CO2

A) 5.29 x 1024 O atoms B) 1.03 x 1022 O atoms C) 1.65 x 1023 O atoms D) 6.01 x 1022 O atoms E) 1.20 x 1023 O atoms A) 5.29 x 1024 O atoms B) 1.03 x 1022 O atoms C) 1.65 x 1023 O atoms D) 6.01 x 1022 O atoms E) 1.20 x 1023 O atoms

Calculate the molar mass, in g/mol, of Fe2(CO3)3.

A) 212.89 g/mol B) 278.58 g/mol C) 281.90 g/mol D) 291.73 g/mol E) None of the above A) 212.89 g/mol B) 278.58 g/mol C) 281.90 g/mol D) 291.73 g/mol E) None of the above

How many moles of NH3 are there in 77.5 g of NH3

A) 0.220 mol B) 4.55 mol C) 14.0 mol D) 1.31 * 103 mol E) None of the above. A) 0.220 mol B) 4.55 mol C) 14.0 mol D) 1.31 * 103 mol E) None of the above.

Balance the following chemical equation: NaNO3 $\rarr$ NaNO2 + O2

A) NaNO3 $\rarr$2NaNO2 + O2 B) 2NaNO3 $\rarr$ NaNO2 + O2 C) NaNO3 $\rarr$ 2NaNO2 + 2O2 D) 2NaNO3 $\rarr$ 2NaNO2 + O2 E) None of the above are balanced A) NaNO3 $\rarr$2NaNO2 + O2 B) 2NaNO3 $\rarr$ NaNO2 + O2 C) NaNO3 $\rarr$ 2NaNO2 + 2O2 D) 2NaNO3 $\rarr$ 2NaNO2 + O2 E) None of the above are balanced

A) is heavier than one mole of lead (Pb). B) is 77.0 g of iron. C) is 26.0 g of iron. D) weighs the same as one mole of lead. E) None of the above. A) is heavier than one mole of lead (Pb). B) is 77.0 g of iron. C) is 26.0 g of iron. D) weighs the same as one mole of lead. E) None of the above.

Phosphorus reacts with iodine as shown in the chemical reaction below. What is the percent yield of the reaction if 28.2 g PI3 is obtained from the reaction of 48.0 g of I2 with excess phosphorus? 2P(s) + 3I2(s) $\rarr$ 2PI3(s)

A) 51.3 % B) 52.3 % C) 53.3 % D) 54.3% E) None of the above A) 51.3 % B) 52.3 % C) 53.3 % D) 54.3% E) None of the above

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO2 and 0.826 g of H2O are produced. What is the empirical formula of the compound

A) C2H3O B) CH4O C) C2H3O3 D) CH3O E) None of the above A) C2H3O B) CH4O C) C2H3O3 D) CH3O E) None of the above

Calculate the average atomic mass of silver using the following data: $\begin{array}{|l|l|l|} \hline \text { Isotope } & \text { Abundance } & \text { Mass } \\ \hline ^{107} \mathrm{Ag} & 51.84 \% & 106.9051 ~\mathrm{amu} \\ \hline ^{109} \mathrm{Ag} & 48.16 \% & 108.9048 ~\mathrm{amu} \\ \hline \end{array}$

A) 106.91 amu B) 108.00 amu C) 107.90 amu D) 107.87 amu E) 108.90 amu A) 106.91 amu B) 108.00 amu C) 107.90 amu D) 107.87 amu E) 108.90 amu

How many O atoms are there in 51.4 g CaSO4

A) 4.00 B) 2.40 * 1024 C) 1.13 D) 9.09 * 1023 E) 2.28 * 1023 A) 4.00 B) 2.40 * 1024 C) 1.13 D) 9.09 * 1023 E) 2.28 * 1023

Exam 3: Mass Relationships in Chemical Reactions

The Hall process for the production of aluminum involves the reaction of aluminum oxide with elemental carbon to give aluminum metal and carbon monoxide. If the yield of this reaction is 75%, what mass of aluminum metal can be produced from the reaction of 1.65 * 10⁶ g of aluminum oxide with 1.50 * 10⁶ g of carbon

(Multiple Choice)

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Question 81

How many O atoms are in 4.39 g of CO₂

(Multiple Choice)

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Question 82

An atom of bromine has a mass about four times greater than that of an atom of neon. How many grams of neon will contain the same number of atoms as 1,000 g of bromine

(Multiple Choice)

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Question 83

Calculate the molar mass, in g/mol, of Fe₂(CO₃)₃.

(Multiple Choice)

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Question 84

How many moles of NH₃ are there in 77.5 g of NH₃

(Multiple Choice)

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Question 85

Balance the following chemical equation: NaNO₃ $\rarr$ NaNO₂ + O₂

(Multiple Choice)

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Question 86

One mole of iron

(Multiple Choice)

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Question 87

Phosphorus reacts with iodine as shown in the chemical reaction below. What is the percent yield of the reaction if 28.2 g PI₃ is obtained from the reaction of 48.0 g of I₂ with excess phosphorus? 2P(s) + 3I₂(s) $\rarr$ 2PI₃(s)

(Multiple Choice)

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Question 88

There are two stable isotopes of chlorine: chlorine-35, with a mass of 34.968853 amu; and chlorine-37, with a mass of 36.965903. Given that the average atomic mass of a chlorine atom is 35.45 amu, which of the following statements is true?

(Multiple Choice)

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Question 89

What is the minimum mass of water necessary to produce 200. g of sulfuric acid in the following reaction 2SO₂ + O₂ + 2H₂O $\rarr$ 2H₂SO₄

(Multiple Choice)

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Question 90

If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in units of g/mol

(Multiple Choice)

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Question 91

Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid. How many total moles of acid are formed when starting with 4.5 g of PCl₅ and excess H₂O? PCl₅ + 4H₂O $\rarr$ 5HCl + H₃PO₄

(Multiple Choice)

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Question 92

What is the coefficient for O₂ when the following combustion reaction of a hydrocarbon is balanced _ C₇H₁₄ + _ O₂ $\rarr$ _ CO₂ + _ H₂O

(Multiple Choice)

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Question 93

The reaction of 60.0 g of aluminum oxide with 30.0 g of carbon produced 22.5 g of aluminum. What is the percent yield for this reaction Al₂O₃ + 3C $\rarr$ 2Al + 3CO

(Multiple Choice)

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Question 94

How many moles of phosphine (PH₃) are produced for every 4.0 moles of hydrogen that react according to the chemical equation below? 3H₂ + P₂ $\rarr$ 2PH₃

(Multiple Choice)

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Question 95

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO₂ and 0.826 g of H₂O are produced. What is the empirical formula of the compound

(Multiple Choice)

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Question 96

Calculate the average atomic mass of silver using the following data: Isotope Abundance Mass 51.84\% 106.9051\nobreakspace 48.16\% 108.9048\nobreakspace

(Multiple Choice)

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Question 97

An unknown compound with a molar mass of 223.94 g/mol consists of 32.18% C, 4.50% H, and 63.32% Cl. Find the molecular formula for the compound.

(Multiple Choice)

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Question 98

A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper (density of Cu = 8.92 g/cm³)

(Multiple Choice)

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Question 99

How many O atoms are there in 51.4 g CaSO₄

(Multiple Choice)

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Question 100

Showing 81 - 100 of 194

Exam 3: Mass Relationships in Chemical Reactions

How many O atoms are in 4.39 g of CO2

An atom of bromine has a mass about four times greater than that of an atom of neon. How many grams of neon will contain the same number of atoms as 1,000 g of bromine

Calculate the molar mass, in g/mol, of Fe2(CO3)3.

How many moles of NH3 are there in 77.5 g of NH3

Balance the following chemical equation: NaNO3 →\rarr→ NaNO2 + O2

One mole of iron

Phosphorus reacts with iodine as shown in the chemical reaction below. What is the percent yield of the reaction if 28.2 g PI3 is obtained from the reaction of 48.0 g of I2 with excess phosphorus? 2P(s) + 3I2(s) →\rarr→ 2PI3(s)

There are two stable isotopes of chlorine: chlorine-35, with a mass of 34.968853 amu; and chlorine-37, with a mass of 36.965903. Given that the average atomic mass of a chlorine atom is 35.45 amu, which of the following statements is true?

What is the minimum mass of water necessary to produce 200. g of sulfuric acid in the following reaction 2SO2 + O2 + 2H2O →\rarr→ 2H2SO4

If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in units of g/mol

Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid. How many total moles of acid are formed when starting with 4.5 g of PCl5 and excess H2O? PCl5 + 4H2O →\rarr→ 5HCl + H3PO4

What is the coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced ___ C7H14 + ___ O2 →\rarr→ ___ CO2 + ___ H2O

The reaction of 60.0 g of aluminum oxide with 30.0 g of carbon produced 22.5 g of aluminum. What is the percent yield for this reaction Al2O3 + 3C →\rarr→ 2Al + 3CO

How many moles of phosphine (PH3) are produced for every 4.0 moles of hydrogen that react according to the chemical equation below? 3H2 + P2 →\rarr→ 2PH3

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO2 and 0.826 g of H2O are produced. What is the empirical formula of the compound

Calculate the average atomic mass of silver using the following data: Isotope Abundance Mass 51.84\% 106.9051\nobreakspace 48.16\% 108.9048\nobreakspace

An unknown compound with a molar mass of 223.94 g/mol consists of 32.18% C, 4.50% H, and 63.32% Cl. Find the molecular formula for the compound.

A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper (density of Cu = 8.92 g/cm3)

How many O atoms are there in 51.4 g CaSO4

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How many O atoms are in 4.39 g of CO₂

Calculate the molar mass, in g/mol, of Fe₂(CO₃)₃.

How many moles of NH₃ are there in 77.5 g of NH₃

Balance the following chemical equation: NaNO₃ $\rarr$ NaNO₂ + O₂

Phosphorus reacts with iodine as shown in the chemical reaction below. What is the percent yield of the reaction if 28.2 g PI₃ is obtained from the reaction of 48.0 g of I₂ with excess phosphorus? 2P(s) + 3I₂(s) $\rarr$ 2PI₃(s)

What is the minimum mass of water necessary to produce 200. g of sulfuric acid in the following reaction 2SO₂ + O₂ + 2H₂O $\rarr$ 2H₂SO₄

Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid. How many total moles of acid are formed when starting with 4.5 g of PCl₅ and excess H₂O? PCl₅ + 4H₂O $\rarr$ 5HCl + H₃PO₄

What is the coefficient for O₂ when the following combustion reaction of a hydrocarbon is balanced _ C₇H₁₄ + _ O₂ $\rarr$ _ CO₂ + _ H₂O

The reaction of 60.0 g of aluminum oxide with 30.0 g of carbon produced 22.5 g of aluminum. What is the percent yield for this reaction Al₂O₃ + 3C $\rarr$ 2Al + 3CO

How many moles of phosphine (PH₃) are produced for every 4.0 moles of hydrogen that react according to the chemical equation below? 3H₂ + P₂ $\rarr$ 2PH₃

When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO₂ and 0.826 g of H₂O are produced. What is the empirical formula of the compound

A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper (density of Cu = 8.92 g/cm³)

How many O atoms are there in 51.4 g CaSO₄