Unit 4 Practice Questions

Unit 4 Practice Questions
Reactions: balancing, types Questions 1-3 refer to the following: 1 2 Cu + HNO Cu(NO3)2 + H2O + NO 4 5 When the above equation is balanced, what will be the coefficient of Cu? If 6 moles of Cu reacted according to the above equation, what will be the number of moles of NO formed? If Cu(NO3)2 goes into solution as ions, what will be the number of ions into which it will dissociate?

Questions 1-3 refer to the following:
NH3 CO2 HCl O2 A gas produced by the reaction of zinc with hydrochloric acid A gas combustion product that is heavier than air A gas produced by the heating of potassium chlorate

One mole of NaCl contains 2 moles of ions II
NaCl is a stable salt at room temperature BECAUSE The reaction in which HgO is heated to release O2 is called decomposition In a decomposition reaction, the original compound is broken apart into equal numbers of atoms BECAUSE Density T,F F,T

Air contains much more nitrogen than oxygen
When a hydrocarbon is combusted in air, carbon monoxide is the major product II Air contains much more nitrogen than oxygen BECAUSE A piece of zinc placed in a blue copper solution will displace the copper from the solution, producing copper metal and a colorless Zn2+ solution Copper is a much more active metal than zinc BECAUSE Density T,F F,T

I A wooden splint is set on fire and blown out, leaving a hot glowing end. When the glowing splint is inserted into a sample of purified CO2 gas, it will reignite into a flame II CO2 gas contains oxygen BECAUSE Density T,F F,T

AgCl is insoluble in water II
All chlorides are soluble in water except for those of silver, mercury and lead BECAUSE Calcium phosphate is a water-soluble compound All group I ions form water-soluble salts BECAUSE Density T,F F,T

The reaction of aluminum with dilute H2SO4 can be classified as
Synthesis Decomposition Single replacement Double replacement Density E

___C4H10 + ___O2 ___CO2 + ___H2O 1,6,4,2 2,13,8,10 1,6,1,5 3,10,16,20
What are the simplest whole-number coefficients that balance this equation? ___C4H10 + ___O ___CO2 + ___H2O 1,6,4,2 2,13,8,10 1,6,1,5 3,10,16,20 4,26,16,20 Density E

___C2H4 + ___O2 ___CO2 + ___H2O 1 2 3 4 5
If the equation for the reaction below is balanced using the smallest possible whole-number coefficients, then the coefficient for oxygen gas is ___C2H4 + ___O ___CO2 + ___H2O 1 2 3 4 5 Density E

___C4H10 + ___O2 ___CO2 + ___H2O 2 4 8 10 13
When the equation below is balanced using the lowest whole-number terms, the coefficient of CO2 is ___C4H10 + ___O ___CO2 + ___H2O 2 4 8 10 13 Density E

___NF3 + ___H2O ___HF + ___NO + ___NO2 0.5 mole 1 mole 2 moles 3 moles
When the equation for the reaction below is balanced, how many moles of NF3 wold be required to react completely with 6 moles of H2O? ___NF3 + ___H2O ___HF + ___NO + ___NO2 0.5 mole 1 mole 2 moles 3 moles 4 moles Density E

Which coefficient balances the reaction given below?
2Ca3(PO4)2 + 6SiO2 + 10C CO + P4 + ___CaSiO3 2 4 5 6 8 Density E

Which of the following reactions produces a yellow precipitate?
NaOH (s) + HCl (aq) NaCl(aq) + H2O 2NaOH(aq) + BaCl2 (aq) Ba(OH)2 (s) + 2NaCl (aq) Pb(NO3)2 (aq) + 2KI (aq) KNO3 (aq) + PbI2 (s) CuO(s) + Mg(s) Cu(s) + MgO (s) 4Fe + 3O Fe2O3 Density E

When the equation for the reaction shown below is completed and balanced and all coefficients are reduced to lowest whole-number terms, the coefficient of O2 is ___Al + ___O ___Al2O3 1 2 3 4 6 Density E

___C6H12O6 + ___O2 ___CO2 + ___H2O 20 38 21 19 18
What is the sum of the coefficients of the following equation when it is balanced? ___C6H12O6 + ___O ___CO2 + ___H2O 20 38 21 19 18 Density E

What is the precipitate produced from the double displacement reaction of an aqueous solution of lead(II) nitrate and an aqueous solution of potassium sulfate? PbSO4 KNO3 K2Pb NO2 SO3 Density E

The reaction below is classified as a
CH3CO2Na + HClO CH3CO2H + NaClO4 Double displacement reaction Synthesis reaction Decomposition reaction Single displacement and decomposition reaction Synthesis and decomposition reaction Density E

The above reaction is classified as a Decomposition
H2 + Cl HCl The above reaction is classified as a Decomposition Double displacement Neutralization Oxidation-reduction Single displacement Density E

__K2Cr2O7 + __HCl __KCl + __CrCl3 + __H2O + __Cl2 10 12 13 14 15
What is the sum of the coefficients of the products for the following reaction, after balancing? __K2Cr2O7 + __HCl __KCl + __CrCl3 + __H2O + __Cl2 10 12 13 14 15 Density E

Which equation is correctly balanced? Na + Cl2 2NaCl
CH4 + 3O CO2 + H2O 2KI + Pb(NO3) KNO3 + PbI2 H2SO4 + KOH K2SO4 + H2O C6H12O6 + 6O CO2 + H2O Density E

Which of the following can be classified as a precipitation reaction?
HCl (aq) + NaOH (aq) KBr (aq) + NaCl (aq) AgNO3(aq) + MgCl2(aq) CaCl2 (aq) + KI (aq) NaNO3 (aq) + HC2H3O2 (aq) Density E

___Cl2 + ___H2O ___HCl +___HClO3 1 3 5 10 12
What would be the stoichiometric coefficient of hydrochloric acid in the following equation? ___Cl2 + ___H2O ___HCl +___HClO3 1 3 5 10 12 Density E

___C2H6 + ___O2 ___CO2 +___H2O
When the equation ___C2H6 + ___O ___CO2 +___H2O Is competely balanced using the lowest whole number coefficients, the sum of the coefficients will be 4 9.5 19 15.5 11 Density E

Which reaction between ions does not form a precipitate?
Ag1+ + Cl1- Pb2+ + 2I1- Ca2+ + CO32- Hg2+ + 2Br1- Na1+ + OH1- Density E

No reaction takes place
The product formed when oxygen and hydrogen are mixed in a test tube at room temperature is Hydrogen peroxide Water A base A zwitterion No reaction takes place Density E

___C2H4 + ___O2 ___CO2 + ___H2O 1 2 3 4 5
If the equation for the reaction below is balanced with whole-number coefficients, what is the coefficient for oxygen gas? ___C2H4 + ___O ___CO2 + ___H2O 1 2 3 4 5 Density E

Higher in the activity series than the metal in solution
For a metal atom to replace another kind of metallic ion in a solution, the metal atom must be A good oxidizing agent Higher in the activity series than the metal in solution Lower in the electromotive chart than the metal in solution Equal in activity to the metal in solution Density E

How many atoms are represented in the formula Ca3(PO4)2?
5 8 9 12 13 Density E

What is the total number of atoms represented in one molecule of (CH3)2NH?
5 8 9 10 12 Density E

The chemical symbol Ar could stand for One mole of argon
One atom of argon Both a mole or an atom of argon Neither a mole or an atom of argon One molecule of argon Density E

Which salt has a solubility that is different from the other four?
AgCl PbBr2 Ca3(PO4)2 Na2CO3 Al(OH)3 Density E

All of the substances above would be in the net ionic equation
The net ionic equation for the reaction between CaCl2 and Na2CO3 to form calcium carbonate and sodium chloride would include all of the following except: Ca2+ CO32- 2Na1+ CaCO3 All of the substances above would be in the net ionic equation Density E

When most fuels burn, the products include carbon dioxide and
Hydrocarbons Hydrogen Water Hydroxide Hydrogen peroxide Density E

Which of the following elements normally exist as monoatomic molecules?
Cl H O N He Density E

The whole number coefficients of the balanced equation are
In this equation: Al(OH)3 + H2SO Al2(SO4)3 + H2O The whole number coefficients of the balanced equation are 1,3,1,2 2,3,2,6 2,3,1,6 1,3,1,6 Density E

For the reaction of sodium with water, the balanced equation using the smallest whole numbers has which of the following coefficients? I. 1 II. 2 III. 3 I only III only I and II only II and III only I, II, and III Density E

The reaction of zinc metal, Zn, and hydrochloric acid, HCl, produces which of the following?
I. H2 (g) II. Cl2 (g) III. Zn2+ (aq) II only III only I and II only I and III only I, II, and III Density E

Which reactions would form at least one solid precipitate as a product
Which reactions would form at least one solid precipitate as a product? Assume aqueous reactants. I. AgNO3 + NaCl NaNO3 + AgCl II. Pb(NO3)2 + 2KI PbI2 + 2KNO3 III. 2NaOH + H2SO Na2SO4 + 2H2O I only II only III only I and II only II and III only Density E

Which of these equations is/are properly balanced?
I. Cl2 + NaBr Br2 + 2NaCl II. 2Na + O Na2O III. 2K + 2H2O H2 + 2KOH I only II only III only I and III only I, II and III Density E

A product is given off as a gas The products can react with each other
One reason for a double displacement reaction to go to completion is that A product is soluble A product is given off as a gas The products can react with each other The products are miscible Density E

II. % Composition, Empirical and Molecular Formulas
The percent composition of oxygen in water is 33% II One atom of oxygen makes up one-third of the mass of a water molecule BECAUSE Density T,F F,T

Laboratory results showed the composition of a compound to be 58
Laboratory results showed the composition of a compound to be 58.81% barium, 13.73% sulfur and 27.46% oxygen. What is the empirical formula? BaSO4 BaS2O Ba2SO3 BaS2O4 Ba2SO4 Conversion D

What is the percent composition of oxygen in C6H12O6 (molar mass = 180)?
25% 33% 40% 53% 75% Conversion D

A compound was analyzed and found to be composed of 75% carbon and 25% hydrogen. What is the empirical formula of this compound? C2H4 CH4 CH3 CH2 CH Conversion D

The percent composition by mass of oxygen in BaSO4 is
233.4% 66.7% 27.4% 58.7% 13.7% Conversion D

Which statement is true about the percent composition by mass in C6H12O6?
Carbon is 6.7% by mass Oxygen is 53.3 % by mass Hydrogen is 12% by mass Carbon is 72% by mass Carbon is 20% by mass Conversion D

What is the approximate percentage composition by mass of the element oxygen in the compound HClO4?
16% 32% 50% 64% 75% Conversion D

The percent composition of an unknown element X in CH3X is 32%
The percent composition of an unknown element X in CH3X is 32%. Which of the following is element X? H F Cl Na Li Conversion D

A compound’s composition by mass is 50% S and 50% O
A compound’s composition by mass is 50% S and 50% O. What is the empirical formula of this compound? SO SO2 S2O S2O3 S3O4 Conversion D

What percentage of the total mass of KHCO3 is made up by nonmetallic elements?
17% 83% 61% 20% 50% Conversion D

A compound has a composition of 40% sulfur and 60% oxygen by mass
A compound has a composition of 40% sulfur and 60% oxygen by mass. What is the empirical formula of this compound? SO S2O3 S2O7 SO3 SO2 Conversion D

A hydrocarbon has the empirical formula CH3
A hydrocarbon has the empirical formula CH3. A probable molecular formula for this compound could be C3H3 C2H6 C3H8 C4H8 C5H10 Conversion D

What is the percentage by mass of sulfur in H2SO4? 16% 33% 36% 42%
Cannot be determined Conversion D

What is the percent composition by weight of Al in Al2(SO4)3?
7.9% 31.6% 15.8% 12.7% 22.3% Conversion D

What is the molecular formula of a compound with the empirical formula C3H6O2 and a mass of 148 amu?
None of the above Conversion D

What is the percent by mass of silicon in a sample of silicon dioxide?
21% 33% 47% 54% 78% Conversion D

Which of the following could be the molecular formula for a molecule with an empirical formula of CH2? CH CH4 C2H2 C2H6 C3H6 Conversion D

I. a given compound can have the same molecular and empirical formula
Which of the following statements about molecular and empirical formulas is/are false? I. a given compound can have the same molecular and empirical formula II. The molecular formula is a whole-number multiple of the empirical formula III. H2O2 represents the empirical formula of hydrogen peroxide III only I and II only II and III only I, II, and III I only Conversion D

What is the percentage composition of calcium in calcium hydroxide, Ca(OH)2?
40% 43% 54% 69% 74% Conversion D

Which of the following compounds contains the greatest percentage of oxygen by weight?
C3H6O5Cl C3H6O2 C5H10O5 C4H8O3 They are all equal Conversion D

What is the mass of nitrogen in a 50
What is the mass of nitrogen in a 50.0 g sample of sodium nitrite (NaNO2)? 20.2 g 16.4 g 10.1 g 8.23 g 23.4 g Conversion D

Mass of hydrate before heating = 250 g
In the laboratory, a sample of hydrated salt was heated at 110oC for 30 minutes until all the water was driven off. The data were as follows: Mass of hydrate before heating = 250 g Mass of hydrate after heating = 160 g From these data, what was the percent of water by mass in the original sample? 26.5 36 47 56 90 Conversion D

What is the approximate percentage of oxygen in the formula mass of Ca(NO3)2?
28 42 58 68 84 Conversion D

What formulas could represent the empirical formula and the molecular formula of a given compound?
CH2O and C4H6O4 CHO and C6H12O6 CH4 and C5H12 CH2 and C3H6 CO and CO2 Conversion D

Analysis of a gas gave: C = 85. 7% and H = 14. 3%
Analysis of a gas gave: C = 85.7% and H = 14.3%. If the formula mass of this gas is 42, what are the empirical formula and the true formula? CH and C4H4 CH2 and C3H6 CH3 and C3H9 C2H2 and C3H6 C2H4 and C3H6 Conversion D

The initial strip of Mg should be cleaned
In synthesizing MgO from a Mg strip burned in a crucible, which of the following is NOT true? The initial strip of Mg should be cleaned The lid of the crucible should fit tightly to exclude oxygen The heating of the covered crucible should continue until the Mg is fully reacted The crucible, lid and contents should be cooled to room temperature before measuring their mass When the Mg appears to be fully reacted, the crucible lid should be partially removed and heating continued Conversion D

A compound whose molecular mass is 90. 0 grams contains 40
A compound whose molecular mass is 90.0 grams contains 40.0% carbon, 6.67% hydrogen, and 53.33% oxygen. What is the true formula of the compound? C2H2O4 CH2O4 C3H6O C3HO3 C3H6O3 Conversion D

If the simplest formula of a substance is CH2 and its molecular mass is 56, what is its true formula? CH2 C2H4 C3H4 C4H8 C5H10 Conversion D

III. Moles, Conversions and Stoichiometry
Questions 1-4 refer to the following: 9.03 x 1023 molecules 44.8 liters 3.5 moles 6.0 grams 3.01 x 1023 atoms 0.25 moles of O2 at STP 3.0 moles of H2 at STP 56 grams of N2 at STP 96.0 grams of SO2 at STP Basic measurements (similar to slide 1) A B C E

One mole of CO2 has a greater mass than 1 mole of H2O
I Two liters of CO2 can be produced by 1 gram of carbon burning completely II The amount of gas evolved in a chemical reaction can be determined by using the mole relationship of the coefficients in the balanced equation BECAUSE One mole of CO2 has a greater mass than 1 mole of H2O BECAUSE The molecular mass of CO2 is greater than the molecular mass of H2O Density T,F F,T

There are 3 moles of atoms in 18 grams of water II
There are 6 x 1023 atoms in 1 mole BECAUSE The complete electrolysis of 45 grams of water will yield 40 grams of H2 and 5 grams of O2 BECAUSE Water is composed of hydrogen and oxygen in a ratio of 8:1 by mass Density T,F F,T

The reaction requires twice as many atoms of chlorine as sodium
When 2 liters of oxygen gas react with 2 liters of hydrogen completely, the limiting factor is the volume of the oxygen II The coefficients in balanced equations of gaseous reactions give the volume relationships of the gases BECAUSE If equal masses of sodium metal and chlorine gas are allowed to react, some sodium will be leftover after all the chlorine is used up The reaction requires twice as many atoms of chlorine as sodium BECAUSE Density T,F F,T

In the following reaction, how many liters of SO2 at STP will result from the complete burning of pure sulfur in 8 liters of oxygen? S + O SO2 1 4 8 16 32 Conversion D

If 80 grams of Al and 80 grams of Fe2O3 are combined, what is the maximum number of moles of Fe that can be produced? 2Al + Fe2O Al2O3 + 2Fe 1 4 8 16 32 Conversion D

How many grams of C2H2 are formed from 0.400 moles of CaC2?
Acetylene, used as a fuel in welding torches, is produced in a reaction between calcium carbide and water: CaC2 + 2H2O Ca(OH)2 + C2H2 How many grams of C2H2 are formed from moles of CaC2? 0.400 0.800 4.00 10.4 26.0 Conversion D

Aspirin (C9H8O4) is prepared by reacting salicylic acid (C7H6O3) and acetic anhydride (C4H6O3)
C7H6O3 + C4H6O C9H8O4 + C2H4O2 How many moles of salicylic acid should be used to prepare six 5-grain aspirin tablets? (1g = 15.5 grains) 0.01 0.1 1.0 2.0 31.0 Conversion D

Ag(NH3) Ag+ + 2NH3 If 5.8 g of Ag(NH3)2+ yields 1.4 g of ammonia, how many moles of silver are produced? 4.4 5.8 0.041 0.054 7.2 Conversion D

How many grams of O2 will it take to oxidize 88 grams of C3H8 to CO and H2O?
32 64 112 166 224 Conversion D

How many molecules are in a 36.5 g sample of SF6 gas?
1.51 x 1022 1.06 x 1022 1.51 x 1023 1.06 x 1024 1.51 x 10-24 Conversion D

What would be the approximate weight of 1.204 x 1024 bromine atoms?
80 grams 120 grams 160 grams 180 grams 200 grams Conversion D

Chlorophyll, a green pigment involved in the light reactions of photosynthesis, consists of percent Mg. If you are given a 100 g sample of chlorophyll, how many atoms of Mg will it contain? 6.02 x 1022 atoms 6.02 x 1023 atoms 6.02 x 1024 atoms 6.02 x 1025 atoms None of the above Conversion D

Water is formed by the addition of 4. 0 g of H2 to an excess of O2
Water is formed by the addition of 4.0 g of H2 to an excess of O2. If 27 g of H2O is recovered, what is the percent yield for the reaction? 25% 50% 75% 100% Cannot be determined Conversion D

In the reaction 2SO2 + O SO3, 0.25 mole of sulfur dioxide is mixed with 0.25 mole of oxygen and allowed to react. What is the maximum number of moles of SO3 that can be produced? mole 0.125 mole 0.25 mole 0.5 mole 1.0 mole Conversion D

The volume of water vapor required to produce 44
The volume of water vapor required to produce 44.8 liters of oxygen by the below reaction is 2H2O H2 + O2 11.2 L 22.4 L 44.8 L 89.6 L 100.0 L Conversion D

Given this reaction that occurs in plants: 6CO2 + 6H2O C6H12O6 + 6O2
If 54 grams of water are consumed by the plant, how many grams C6H12O6 can be made? Assume an unlimited supply of carbon dioxide for the plant to consume as well. 54 grams 180 grams 540 grams 3 grams 90 grams Conversion D

According to the reaction: Pb + S PbS
When 20.7 grams of lead are reacted with 6.4 grams of sulfur There will be an excess of 20.7 grams of lead The sulfur will be in excess by 3.2 grams The lead and sulfur will react completely without any excess reactants The sulfur will be the limiting factor in the reaction There will be an excess of 10.3 grams of lead Conversion D

None of the above statements is correct.
Given a 4-gram sample of each H2(g) and He(g), each in separate containers, which of the following statements is true? (assume STP) The sample of hydrogen gas will occupy 44.8 liters and the sample of helium will contain 6.02 x 1023 molecules The sample of hydrogen gas will occupy 22.4 liters and sample of helium will contain 3.02 x 1023 molecules The sample of hydrogen gas will occupy 44.8 liters and the sample of helium will contain x 1024 molecules The sample of helium will occupy 44.8 liters and the sample of hydrogen gas will contain 6.02 x 1023 molecules None of the above statements is correct. Conversion D

If 48.6 grams of magnesium are placed in a container with 64 grams of oxygen gas and the reaction below proceeds to completion, what is the mass of MgO (s) produced? 2Mg + O MgO 15.4 grams 32.0 grams 80.6 grams 96.3 grams 112 grams Conversion D

Given the reaction at STP: Mg + 2HCl MgCl2 + H2
How many liters of H2 can be produced from the reaction of grams of Mg with excess HCl? 2.0 liters 4.0 liters 11.2 liters 22.4 liters 44.8 liters Conversion D

Have a molar mass of 20.0 grams/mole and occupy 11.2 liters
A sample of a gas at STP contains 3.01 x 1023 molecules and has a mass of 20.0 grams. This gas would Have a molar mass of 20.0 grams/mole and occupy 11.2 liters Occupy 22.4 liters and have a molar mass of 30.0 grams/mole Occupy 22.4 liters and have a molar mass of 20.0 grams/mole Have a molar mass of 40.0 grams/mole and occupy 33.6 liters Have a molar mass of 40.0 grams/mole and occupy 11.2 liters Conversion D

If 1 mole of H2 is consumed, 0.5 mole of N2 is produced
2NO + 2H N2 + 2H2O Which of the following statements is true regarding the reaction given above? If 1 mole of H2 is consumed, 0.5 mole of N2 is produced If 1 mole of H2 is consumed, 0.5 mole of H2O is produced If 0.5 mole of H2 is consumed, 1 mole of N2 is produced If 0.5 mole of H2 is consumed, 1 mole of NO is consumed If 0.5 mole of H2 iscondsumed, 1 mole of H2O is produced Conversion D

Propane and oxygen react according to the equation: C3H8 + 5O2 3CO2 + 4H2O
How many grams of water can be produced from the complete combustion of 2.0 moles of C3H8? 144.0 82.0 8.0 44.8 22.4 Conversion D

Carbon and oxygen react to form carbon dioxide according to the reaction: C + O2 CO2
How much carbon dioxide can be formed from the reaction of 36 grams of carbon with 64 grams of oxygen gas? 36 grams 64 grams 28 grams 132 grams 88 grams Conversion D

How many grams of Fe2O3 can be formed form the rusting of 446 grams of Fe according to the reaction: 4Fe + 3O Fe2O3 320 grams 223 grams 159 grams 480 grams 640 grams Conversion D

Cl2 is the excess reagent and 5.0 moles of NaCl will be produced
Sodium and chlorine react according to the following reaction: 2Na + Cl NaCl If the reaction starts with 5.0 moles of Na and 3.0 moles of Cl2, then which statement below is true? Cl2 is the excess reagent and 5.0 moles of NaCl will be produced Na is the excess reagent and 2.5 moles of NaCl will be produced There will be an excess of 2.0 moles of Na Na is the limiting reagent and 2.0 moles of NaCl will be produced Cl2 is the excess reagent and 2.0 moles of NaCl will be produced Conversion D

According to the reaction: 3H2 + N2 2NH3
How many grams of hydrogen gas and nitrogen gas are needed to make exactly 68 grams of ammonia? 2 grams of hydrogen gas and 28 grams of nitrogen gas 3 grams of hydrogen gas and 1 gram of nitrogen gas 12 grams of hydrogen gas and 56 grams of nitrogen gas 102 grams of hydrogen gas and 34 grams of nitrogen gas 6 grams of hydrogen gas and 2 grams of nitrogen gas Conversion D

What is the mass of 3.0 x 1023 atoms of neon gas? 0.50 grams 1.0 grams
Conversion D

It is the conversion factor between grams and atomic mass units
Which of the following statements is the most accurate with regard to the significance of Avogadro’s number, 6.02 x 1023? It is the conversion factor between grams and atomic mass units It is a universal physical constant just as the speed of light It is the number of particles that is required to fill a 1-liter container It is the inverse diameter of an H atom It is the number of electrons in the universe Conversion D

mass of crucible and cover 31.623 g
In the laboratory a student was determining the formula for the hydrate of barium chloride, BaCl2. The student heated the sample in the crucible strongly for 10 minutes. The mass data is provided below: mass of crucible and cover g mass of crucible, cover and g sample prior to heating mass of crucible, cover and g sample after heating After the heating, how many moles of water were removed from the sample? moles moles 0.112 moles 0.256 moles 1.85 moles Conversion D

How many grams of hydrogen gas can be produced from the following reaction if 65 grams of zinc and 65 grams of HCl are present in the reaction? Zn + 2HCl ZnCl2 + H2 1.0 1.8 3.6 7.0 58 Conversion D

If 60. grams of NO is reacted with sufficient O2 to form NO2 that is removed during the reaction, how many grams of NO2 can be produced? 46 60. 92 120 180 Conversion D

What volume of gas, in liters, would 1
What volume of gas, in liters, would 1.5 moles of hydrogen occupy at STP? 11.2 22.4 33.6 44.8 67.2 Conversion D

A gas at STP that contains 6
A gas at STP that contains 6.02 x 1023 atoms and forms diatomic molecules will occupy 11.2 L 22.4 L 33.6 L 67.2 L 1.06 qt Conversion D

5. 00 liters of gas at STP have a mass of 12. 5 grams
5.00 liters of gas at STP have a mass of 12.5 grams. What is the molar mass of the gas? 12.5 g/mol 25.0 g/mol 47.5 g/mol 56.0 g/mol 125 g/mol Conversion D

How many moles of CaO are needed to react with an excess of water to form 370 grams of calcium hydroxide? 1.0 2.0 3.0 4.0 5.0 Conversion D

1 mol of Cl- ions and 1 mol of Br- 1 mol of Cl- ions and 2 mol of Br-
When 1 mole of chlorine gas reacts completely with excess KBr solution, as shown below, the products obtained are Cl2 + 2Br- 1 mol of Cl- ions and 1 mol of Br- 1 mol of Cl- ions and 2 mol of Br- 1 mol of Cl- ions and 1 mol of Br2 2 mol of Cl- ions and 1 mol of Br2 2 mol of Cl- ions and 2 mol of Br2 Conversion D

What mass of CaCO3 is needed to produce 11
What mass of CaCO3 is needed to produce 11.2 liters of CO2 at STP when the calcium carbonate is reacted with an excess amount of hydrochloric acid? 25.0 g 44.0 g 50.0 g 100. g None of the above Conversion D

What is the approximate formula mass of Ca(NO3)2? 70 82 102 150 164
Conversion D

If 10 liters of CO gas react with sufficient oxygen for a complete reaction, how many liters of CO2 gas are formed? 5 10 15 20 40 Conversion D

None of either compound 20. g NaOH 40. g NaOH 60. g NaOH
If 49 grams of H2SO4 react with 80.0 grams of NaOH, how much reactant will be left over after the reaction is complete? 24.5 g H2SO4 None of either compound 20. g NaOH 40. g NaOH 60. g NaOH Conversion D

Given one mole of CH4 (g) at STP. Which statements are true?
I. There are 6.02 x 1023 molecules present II. The sample will occupy 22.4 L III. The sample will weigh 16 g I only II only I and III only II and III only I, II, and III Conversion D

What is the molar mass of Ca3(PO4)2? 310 grams/mole 154 grams/mole
Conversion D

If the density of a diatomic gas at STP is 1
If the density of a diatomic gas at STP is 1.43 g/L, what is the gram molecular mass of the gas? 14.3 g 32.0 g 48.0 g 64.3 g 224 g Conversion D

From 2 moles of KClO3 how many liters of O2 can be produced at STP by decomposition of tall the KClO3? 11.2 22.4 33.6 44.8 67.2 Conversion D

How many atoms are in one mole of water? 3 54 6.02x1023 2(6.02x1023)
Conversion D

Four grams of hydrogen gas at STP contain 6.02x1023 atoms
1.2x1023 molecules 12.04x1023 molecules Conversion D

How many liters of O2 can be produced by completely decomposing 2
How many liters of O2 can be produced by completely decomposing 2.00 moles of KClO3? 11.2 22.4 33.6 44.8 67.2 Conversion D

If the molecular mass of NH3 is 17, what is the density of this compound at STP?
0.25 g/L 0.76 g/L 1.52 g/L 3.04 g/L 9.11 g/L Conversion D

How many grams of sulfur are present in 1 mole of H2SO4?
32 49 64 98 Conversion D

What is the approximate mass, in grams, of 1 liter of nitrous oxide, N2O, at STP?
11.2 22 4 Conversion D

What is the molar mass of CaCO3? 68 g/mol 75 g/mol 82 g/mol 100 g/mol
Conversion D

What volume, in liters, will be occupied at STP by 4 grams of H2?
11.2 22.4 33.6 44.8 56.0 Conversion D

What volume, in liters, of NH3 is produced when 22
What volume, in liters, of NH3 is produced when 22.4 liters of N2 are made to combine completely with a sufficient quantity of H2 under appropriate conditions? 11.2 22.4 44.8 67.2 89.6 Conversion D

What volume, in liters, of SO2 will result from the complete burning of 64 grams of sulfur?
2.0 11.2 44.8 126 158 Conversion D

How many grams of CO2 can be prepared from 150 grams of calcium carbonate reacting with an excess of hydrochloric acid solution? 11 22 33 44 66 Conversion D

What is the mass, in grams, of 1 mole of KAl(SO4)2 .12H20? 132 180 394
474 516 Conversion D

What mass of aluminum will be completely oxidized by 2 moles of oxygen at STP?
Conversion D

In this reaction: CaCO3 + 2HCl CaCl2 + H2O + CO2
If 4.0 moles of HCl are available to the reaction with an unlimited supply of CaCO3, how many moles of CO2 can be produced at STP? 1.0 1.5 2.0 2.5 3.0 Conversion D

The following reaction occurs at STP: 2H2O 2H2 + O2
How many liters of hydrogen gas can be produced by the breakdown of 72 grams of water? 5.6 liters 11.2 liters 22.4 liters 44.8 liters 89.6 liters Conversion D

A sample of a gas at STP contains 3
A sample of a gas at STP contains 3.01 x 1023 molecules and has a mass of 22.0 grams. This gas is most likely CO2 O2 N2 CO NO Conversion D

The number of oxygen atoms in 0.50 mole of Al2(CO3)3 is 4.5 x 1023
Conversion D

4. 0 grams of hydrogen are ignited with 4. 0 grams of oxygen
4.0 grams of hydrogen are ignited with 4.0 grams of oxygen. How many grams of water can be formed? 0.50 2.5 4.5 8.0 36 Conversion D

Unit 4 Practice Questions

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Unit 4 Practice Questions

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