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Exam 3: Mass Relationships in Chemical Reactions

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Question 1

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What is the mass of 0.0250 mol of P₂O₅?

A) 35.5 g
B) 5676 g
C) 0.0250 g
D) 1.51 * 10²² g
E) 3.55 g

F) A) and E)
G) A) and D)

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Question 2

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How many moles of oxygen atoms are there in 10 moles of KClO₃?

A) 3 mol
B) 3.3 mol
C) 10 mol
D) 30 mol
E) 6.02 * 10²⁴ mol

F) None of the above
G) C) and D)

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Question 3

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Calculate the percent composition by mass of oxygen in Na₂CO₃.

Formaldehyde has the formula CH₂O. How many molecules are there in 0.11 g of formaldehyde?

What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 mole of V₂O₅ with 6.0 mole of calcium based on the following chemical reaction? V₂O₅(s) + 5Ca(l) $\rarr$ 2V(l) + 5CaO(s)

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 82% and aluminum ore is 71% by mass aluminum oxide, what mass of aluminum ore must be mined in order to produce 1.0 * 10³ kg (1 metric ton) of aluminum metal by the Hall process?

Vanadium(V) oxide reacts with calcium according to the chemical equation below.When 10.0 moles of V₂O₅ are mixed with 10.0 moles of Ca, which is the limiting reagent? V₂O₅(s) + 5Ca(l) $\rarr$ 2V(l) + 5CaO(s)

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?

Balance the following chemical equation: Al(s)+ Co(NO₃)₂(aq) $\rarr$ Al(NO₃)₃(aq)+ Co(s)

A 0.8715 g sample of sorbic acid, a compound first obtained from the berries of a certain ash tree, is burned completely in oxygen to give 2.053 g of carbon dioxide and 0.5601 g of water.The empirical formula of sorbic acid is

Commonly used gases in the laboratory are generally obtained from pressurized metal gas cylinders, but for small amounts of occasionally used gases, it is sometimes easier just to prepare them chemically as needed.For example, nitrogen monoxide, NO(g), can be prepared in the lab by the following chemical reaction: 3Cu(s)+ 8HNO₃(aq) $\rarr$ 2NO(g)+ 3Cu(NO₃)₂(aq)+ 4H₂O(l) If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO₃, how many moles of NO(g)would be produced, assuming a 75% yield.

Balance the equation below using the smallest set of whole numbers. What is the coefficient of H₂O? ___ PCl₃(l) + ___ H₂O(l) $\rarr$ ___ H₃PO₃(aq) + ___ HCl(aq)

The first step in the Ostwald process for producing nitric acid is 4NH₃(g) + 5O₂(g) $\rarr$ 4NO(g) + 6H₂O(g) . If the reaction of 150.g of ammonia with 150.g of oxygen gas yields 87.g of nitric oxide (NO) , what is the percent yield of this reaction?

What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V₂O₅ with 40.0 g of calcium based on the following chemical reaction? V₂O₅(s) + 5Ca(l) $\rarr$ 2V(l) + 5CaO(s)

Commonly used gases in the laboratory are generally obtained from pressurized metal gas cylinders, but for small amounts of occasionally used gases, it is sometimes easier just to prepare them chemically as needed.For example, nitrogen monoxide, NO(g), can be prepared in the lab by 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.

How many moles of HCl are represented by 1.0 * 10¹⁹ HCl molecules?

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?

How many sodium atoms are there in 6.0 g of Na₃N?

Calculate the mass of FeS formed when 9.42 g of iron reacts with 8.50 g of sulfur according to the following reaction. Fe(s) + S(s) $\rarr$ FeS(s)

How many Mg atoms are present in 170 g of Mg?