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Exam 3: Mass Relationships in Chemical Reactions

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Question 41

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How many sulfur atoms are there in 21.0 g of Al₂S₃

A) 8.42 * 10²² atoms
B) 2.53 * 10²³ atoms
C) 2.14 * 10²³ atoms
D) 6.02 * 10²³ atoms
E) 6.30 * 10²⁶ atoms

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Question 42

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Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory. At times it can be easier to chemically prepare occasionally used gases. For example, nitrogen monoxide, NO(g) , can be prepared in the lab using the following chemical reaction: 3Cu(s) + 8HNO₃(aq) $\rarr$ 2NO(g) + 3Cu(NO₃) ₂(aq) + 4H₂O(l) If 5.0 g of copper metal was added to an aqueous solution containing 2.5 moles of HNO₃, how many moles of NO(g) would be produced, assuming a 100% yield

A) 0.042 mole NO
B) 0.052 mole NO
C) 0.062 mole NO
D) 0.72 mole NO
E) None of the above

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Question 43

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Hydrogen chloride gas can be prepared by the following reaction: 2NaCl(s) + H₂SO₄(aq) $\rarr$ 2HCl(g) + Na₂SO₄(s) How many grams of HCl can be prepared from 2.00 mol H₂SO₄ and 2.56 mol NaCl

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

Balance the following chemical equation: P₄O₁₀ + H₂O $\rarr$ H₃PO₄

The definition of a mole is an Avogadro's number of a specific entity, such as an atom or molecule.

A compound with a percent composition by mass of 24.61% C, 2.75% H, and 72.64% Cl has a molar mass of 292.82 g/mol. What is the empirical formula of the compound

Chlorine gas reacts with phosphorus to produce phosphorus pentachloride. How many grams of PCl₅ are produced from 3.5 g of Cl₂ and excess P 5Cl₂(g) + 2P(s) $\rarr$ 2PCl₅(s)

The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The molar mass of this compound is 284.5 g/mol. What is the molecular formula of the compound

Calculate the mass of N in 2.34 g of N₂H₄

How many fluorine atoms are there in 65 g of CF₄

Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory. At times, it can be easier to chemically prepare occasionally used gases. For example, oxygen gas can be prepared by heating KMnO₄(s) according to the following chemical reaction: 2KMnO₄(s) $\rarr$ K₂MnO₄(s) + MnO₂(s) + O₂(g) How many grams of KMnO₄ would you need to produce 0.27 $\underline{\text{moles}}$ of O₂, assuming 100% conversion? The molar mass of KMnO₄ is 158.034 g/mol.

Refer to the (unbalanced) equation CS₂ + CaO $\rarr$ CO₂ + CaS. How many grams of CaO are required to react completely with 38 g of CS₂

What is the molecular mass of nicotine, C₁₀H₁₄N₂

What is the coefficient of O₂ when the following equation is properly balanced? ___ CH₃OH + ___ O₂ $\rarr$ ___ CO₂ + ___ H₂O

A method for producing pure copper metal involves the reaction of copper(I) sulfide with oxygen gas to give copper metal and sulfur dioxide. Suppose the yield of this reaction is 87%. What mass of a copper ore consisting of 46% copper(I) sulfide must be mined in order to produce 1.0 *10³ kg (1.0 metric ton) of copper metal

How many moles of CF₄ are there in 171 g of CF₄

Calculate the percent composition by mass of sodium in Na₂CO₃.

A compound was discovered whose composition by mass is 85.6% C and 14.4% H. Which of the following could be the molecular formula of this compound

What is the mass of 8.25 * 10¹⁹ UF₆ molecules