Deck 1: Fundamental Concepts of Chemistry

Question 1

Recognize elemental symbols and names of the elements, and name compounds from molecular pictures.

Answer 1

Properties of molecules (the microscopic level) translate into properties of materials (the macroscopic level).

Question 2

Recognize the SI units commonly used in chemistry, and perform some common unit conversions.

Answer 2

The correct conversion ratio leads to cancellation of unwanted units. Proper use of significant figures is important to tell the reader what the accuracy and precision of the measurement are.

Question 3

Analyze and solve problems in a consistent, organized fashion.Solving Quantitative ProblemsStep 1. Determine what is asked for.Step 2. Visualize the problem.Step 3. Organize the data.Step 4. Identify a process to solve the problem.Step 5. Manipulate the equations.Step 6. Substitute and calculate.Step 7. Does the result make sense?

Answer 3

NOT ANSWER

Question 4

Solve mass-number-molar mass-type problems.

Question 5

Perform mole-mass-number conversions.

Question 6

Calculate concentrations of solutions and of diluted solutions.

Question 7

Balance chemical reactions.

Question 8

Calculate the amount of a product from the amounts of the reactants and a balanced chemical equation.

Question 9

Calculate yields of chemical reactions.

Question 10

Solve limiting-reagent-type problems.

Question 11

Which of the following is a microscopic property?

A) the colour of a substance
B) the density of a substance
C) the arrangement of atoms in the molecules making up the substance
D) the mass of a substance
E) the shape of the crystals in a solid substance

Question 12

What is the correct formula for molecular oxygen?

A) O
B) 2O
C) O₂
D) O²
E) O₃

Question 13

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) ?r^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1
yard = 3 ft; 1 gal = 3.785 L; ?C = 5/9 (?F - 32)
proton $\quad$ charge = +1.6022 x 10^-19 C $\quad$ mass = 1.6726 x 10^-27 kg
electron $\quad$ charge = -1.6022 x 10^-19 C $\quad$ mass = 9.1094 x 10^-31 kg
neutron $\quad$ charge = 0 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ mass = 1.6749 x 10^-27 kg

-Which of the following are valid conversions from cubic yards to mm³?

A)
B)
C)
D)
E)

Question 14

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) ?r^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1
yard = 3 ft; 1 gal = 3.785 L; ?C = 5/9 (?F - 32)
proton $\quad$ charge = +1.6022 x 10^-19 C $\quad$ mass = 1.6726 x 10^-27 kg
electron $\quad$ charge = -1.6022 x 10^-19 C $\quad$ mass = 9.1094 x 10^-31 kg
neutron $\quad$ charge = 0 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ mass = 1.6749 x 10^-27 kg

-One less common temperature unit is the Rankine. This scale has the same magnitude degree increment as the Fahrenheit scale, but zero Rankine is the same as absolute zero, or 0 K. Absolute zero is -459.7° Fahrenheit. Which of the following are true?

A) Water freezes at 32 Rankine and boils at 212 Rankine.
B) Water freezes at 273 Rankine and boils at 373 Rankine.
C) Room temperature, 25°C, is 536.7 Rankine.
D) Room temperature, 25°C, is 563.7 Rankine.
E) Body temperature, 37°C, is 563.7 Rankine.

Question 15

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) ?r^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1
yard = 3 ft; 1 gal = 3.785 L; ?C = 5/9 (?F - 32)
proton $\quad$ charge = +1.6022 x 10^-19 C $\quad$ mass = 1.6726 x 10^-27 kg
electron $\quad$ charge = -1.6022 x 10^-19 C $\quad$ mass = 9.1094 x 10^-31 kg
neutron $\quad$ charge = 0 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ mass = 1.6749 x 10^-27 kg

-The distance between two atoms was determined to be 11.4 nm. What is this distance in centimetres?

A) 1.14 x 10^-6 cm
B) 11. 4 x 10⁷ cm
C) 114 cm
D) 0.000000114 cm
E) 1.14 x 10^-11 cm

Question 16

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) ?r^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1
yard = 3 ft; 1 gal = 3.785 L; ?C = 5/9 (?F - 32)
proton $\quad$ charge = +1.6022 x 10^-19 C $\quad$ mass = 1.6726 x 10^-27 kg
electron $\quad$ charge = -1.6022 x 10^-19 C $\quad$ mass = 9.1094 x 10^-31 kg
neutron $\quad$ charge = 0 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ mass = 1.6749 x 10^-27 kg

-Four different target shooters fired five shots at targets and their results are shown below. Which of the following statements best describes the precision and accuracy of each "marksman"?

A) A is accurate and precise, C is inaccurate and precise.
B) B is imprecise and inaccurate, D is accurate and imprecise.
C) A and D have similar precision but A is more accurate.
D) C and D have similar accuracy, but D is more precise.

Question 17

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) ?r^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1
yard = 3 ft; 1 gal = 3.785 L; ?C = 5/9 (?F - 32)
proton $\quad$ charge = +1.6022 x 10^-19 C $\quad$ mass = 1.6726 x 10^-27 kg
electron $\quad$ charge = -1.6022 x 10^-19 C $\quad$ mass = 9.1094 x 10^-31 kg
neutron $\quad$ charge = 0 $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ mass = 1.6749 x 10^-27 kg

-What is the answer, with the correct number of significant figures, for the following problem?3.784 g + 56.3 g + 445.55 g =?

A) 505.634 g
B) 505.63 g
C) 505.6 g
D) 505 g
E) 506 g

Question 18

Use the following information for Questions
1 mole = 6.022 x10²³ particles

-If you had a 50 g sample of C, Al, Fe, Au, and Ti, you would have more atoms of which element?

A) C
B) Al
C) Fe
D) Au
E) Ti

Question 19

Use the following information for Questions
1 mole = 6.022 x10²³ particles

-If you had a 5.0 g sample of Li, Na, K, Rb, and Cs, you would have more atoms of which element?

A) Li
B) Na
C) K
D) Rb
E) Cs

Question 20

Use the following information for Questions
1 mole = 6.022 x10²³ particles

-How many atoms are present in 52.0 grams of iron?

A) 0.93 atoms
B) 5.61 x 10²³
C) 5.61
D) 52
E) 1.20 x 10²⁴

Question 21

Use the following information for Questions
1 mole = 6.022 x10²³ particles

-Consider three mole samples of C, Al, Fe, Au, and Ti; which sample will have the greatest mass?

A) C
B) Al
C) Fe
D) Au
E) Ti

Question 22

How many moles of carbon are present in 20 grams of C₃H₈?

A) 0.40 moles C
B) 0.80 moles C
C) 1.40 moles C
D) 1.67 moles C
E) 3 moles C

Question 23

The line structure is shown below for terephthalic acid, a starting material of Kevlar that is used in bullet proof vests: What is the correct molecular formula for this compound?

A) C₆H₆ O₄
B) C₈H₂ O₄
C) C₈H₆O₄
D) C₁₀H₄O₄
E) C₁₂H₆O₄

Question 24

Cumene is an important industrial chemical used in the manufacture of acetone and phenol. The line structure is shown below: What is the correct molecular formula for cumene?

A) C₈H₁₂
B) C₉H₁₁
C) C₉H₁₂
D) C₁₀H₁₀
E) C₉H₁₆

Question 25

Adipic acid, whose line structure is shown below, is used in the manufacture of nylon used in carpet fibre, among other things. What is the chemical formula for adipic acid?

A) C₄H₂O₄
B) C₆H₂O₄
C) C₆H₆O₄
D) C₆H₈O₄
E) C₆H₁₀O₄

Question 26

Calculate the molar mass of terephthalic acid, whose line structure appears below:

A) 166.13 g/mole
B) 150.13 g/mole
C) 152.12 g/mole
D) 178.14 g/mole
E) 201.14 g/mole

Question 27

Calculate the molar mass of ammonium phosphate, (NH₄)₃PO₄.

A) 94.97 g/mole
B) 18.04 g/mole
C) 113.01 g/mole
D) 131.05 g/mole
E) 149.09 g/mole

Question 28

Calculate the molar mass of potassium carbonate, K₂CO₃

A) 39.10 g/mole
B) 60.01 g/mole
C) 99.11 g/mole
D) 138.211 g/mole
E) 177.31 g/mole

Question 29

Styrene is used in many plastic products and also in automobile tire rubber. The line structure is shown below: How many hydrogen atoms are contained in 1.05 x 10⁶ kg of styrene?

A) 4.86 x 10³¹
B) 6.07 x 10³⁰
C) 1.01 x 10⁷
D) 104
E) 7.71 x 10¹⁵

Question 30

One litre of air contains about 1 x 10^-2 moles of O₂.What is the mass of O₂ contained in a room 10 m long by 5 m wide by 3 m high?

A) 4.8 g
B) 50g
C) 52 kg
D) 48 kg
E) 1500 g

Question 31

How many grams of AgNO₃ need to be added to 400 ml of water to make a solution of 0.250 M concentration?

A) 1.70 g
B) 17.0 g
C) 4.25 g
D) 42.5 g
E) 68.0 g

Question 32

Nitric acid is a corrosive acid capable of dissolving many metals, with the evolution of brown nitrogen dioxide gas as a byproduct. It is often sold as concentrated nitric acid which has [HNO₃] = 16. M. A common concentration used in the laboratory is 6.0 M HNO₃. If you need 20. L of 6.0 M HNO₃, what volume of concentrated nitric acid is required?

A) 6.7 L
B) 7.5 mL
C) 0.75 L
D) 5.7 L
E) 7.5 L

Question 33

Nitric acid, HNO₃, is produced along with water by the reaction of oxygen, O₂, with ammonia, NH₃, and water, H₂O, in a series of steps, with the unbalanced net reaction shown below.
__ NH₃ + __ O₂ $\rarr$ __ HNO₃ + __H₂O
If the coefficient of NH₃ is 1 in the balanced chemical equation of the reaction, what is the coefficient on O₂?

A) 2
B) 3
C) 4
D) 5
E) 6

Question 34

Fertilizer is manufactured from, among other components, phosphoric acid, H₃PO₄, which, itself is primarily synthesized from fluorapetite, Ca₅F(PO₄)₃ and sulphuric acid, H₂SO₄.__ H₂SO₄ + __ Ca₅F(PO₄)₃ $\rarr$ __ H₃PO₄ + __ CaSO₄ + __ HFIf the coefficient of H₂SO₄ is 5 in the balanced chemical equation of the reaction, what is the coefficient of HF?

A) 1
B) 2
C) 3
D) 4
E) 5

Question 35

Two important industrial chemicals, NaOH and chlorine, are produced from solutions of sodium chloride by the following reaction:
__ NaCl + __ H₂O $\rarr$ __ NaOH + __ Cl₂ + __ H₂
If the coefficient of H₂O is 2 in the balanced chemical equation of reaction, what is the coefficient of NaOH?

A) 1
B) 2
C) 3
D) 4
E) 5

Question 36

A 1.345 g sample of solid residue from a hazardous waste dump is being analyzed for barium. The sample is dissolved and then sodium sulphate is added. The insoluble barium sulphate is dried, and a total of 73.8 mg of BaSO₄ is collected. What percent of the sample is barium?

A) 0.323 % Ba
B) 2.33 % Ba
C) 3.23 % Ba
D) 4.02 % Ba
E) 5.23 % Ba

Question 37

Sodium sulphate is used in detergents and can be synthesized by the following unbalanced reaction:
NaCl + H₂SO₄ $\rarr$ Na₂SO₄ + HCl
How much sulphuric acid (in kg) would be required to consume 5.0 x 10³ kg of NaCl?

A) 4.3 x 10⁶ kg
B) 4.2 x10³ kg
C) 4.4 x 10⁴ kg
D) 5.0 x 10⁶ kg
E) 8.7 x 10⁴ kg

Question 38

Aluminum sulphate is used in sand paper, among other uses. How many g of aluminum oxide dihydrate will be needed to produce 500 g of aluminum sulphate by the (unbalanced) reaction below?
Al₂O₃ •2H₂O + H₂SO₄ $\rarr$ Al₂(SO₄)₃ + H₂O

A) 1.46
B) 40.0
C) 202
D) 342
E) 500

Question 39

The industrial synthesis of methanol, CH₃OH, is catalyzed by metal oxides. Billions of kg are produced annually for use in polymers and fuel additives.
CO + 2 H₂ $\rarr$ CH₃OH
How many kg of hydrogen will be required to produce 1.0 x 10⁵ kg of methanol?

A) 3.1 x 10⁶
B) 6.2 x 10³
C) 6.2 x 10⁶
D) 1.3 x 10⁷
E) 1.3 x 10⁴

Question 40

A way of generating dry O₂ in the lab is to heat potassium chlorate. If you determined that 25 grams of O₂ are needed, how much potassium chlorate do you need to start with?

A) 64 grams
B) 96 grams
C) 17 grams
D) 25 grams
E) 128 grams

Question 41

Urea is used as a source of nitrogen in fertilizer. The second step of the synthesis is heating the intermediate ammonium carbamate to produce urea shown in the equation below:
NH₂CO₂ $\rarr$ NH₄ O)NH₂ + H₂O
The reaction proceeds in 60% yield, on average, and the product is mixed with unreacted starting materials, which are readily separated from the product. They can then be recycled and undergo the process again. If one starts with 1 kg of ammonium carbamate, how many times will it have to be cycled through this reaction to give at least a 90% yield?

A) 2
B) 3
C) 4
D) 5
E) infinite number of times

Question 42

How many kg of ethylene oxide is needed to produce 1.05 x 10⁴ kg of ethylene glycol by the following reaction that proceeds in 95% yield?

A) 1.69 x 10⁵
B) 1.78 x 10⁵
C) 5.23 x 10³
D) 7.45 x 10³
E) 7.84 x10³

Question 43

A way of generating dry O₂ in the lab is to heat potassium chlorate. If you determined that 25 grams of O₂ are needed, how much potassium chlorate do you need to start with if there is only a 60% yield?

A) 64 grams
B) 96 grams
C) 17 grams
D) 25 grams
E) 106 grams

Question 44

Hydrazine (N₂H₄) is made by the reaction of ammonia (NH₃) with hypochlorite (OCl^-). Given the following equation 420 kg of ammonia is reacted with excess hypochlorite to generate 315 kg of hydrazine. What is the percent yield for this unbalanced reaction?
NH₃ + OCl^- $\rarr$ N₂H₄ + Cl^- + H₂O

A) 75.0 %
B) 79.7 %
C) 150 %
D) 20.3 %
E) 66.7 %

Question 45

Adiponitrile is produced by the reaction of HCN and butadiene: If 450 kg of butadiene and 400 kg of HCN were to react to completion, what is the maximum amount of adiponitrile that would be produced?

A) 450 kg
B) 8.32 x 10³ moles
C) 1.48 x 10³ moles
D) 800 kg
E) 900 kg

Question 46

Aluminum sulphate is used in finishing paper, among other uses. If 500 kg of aluminum oxide dihydrate react completely with 1500 kg of 90% by mass aqueous H₂SO₄, how many kg of aluminum sulphate can be produced?
Al₂O₃ •2H₂O + 3H₂SO₄ $\rarr$ Al₂(SO₄)₃ + 5H₂O

A) 1.24 x 10³ kg
B) 1.35 x 10³ kg
C) 1.57 x10³ kg
D) 3.62 x10³ kg
E) 4.59 x10³ kg

Question 47

Thermite is a reaction that was once used to weld railroads together as shown below. A 48.0 g sample of Al(s) was reacted with 99.0 g of Fe₂O₃ according to the equation below. What could be the theoretical yield of Fe_(s) in grams?
2 Al_(s) + Fe₂O_3(s) $\rarr$ Al₂O_3(s) + 2 Fe_(s)

A) 52.5 g
B) 99.3 g
C) 69.2 g
D) 48.0 g
E) 175 g

Question 48

Potassium permanganate reacts with hydrochloric acid to give chlorine gas according to unbalanced chemical reaction shown below. If 34.2 g of KMnO₄ were mixed with 0.990 moles of HCl, how many moles of chlorine gas could be produced?
KMnO₄ + HCl $\rarr$ MnCl₂ + KCl + Cl_2(g) + H₂O

A) 0.541 moles
B) 0.850 moles
C) 0.309 moles
D) 0.989 moles
E) 0.354 moles

Question 49

What are the symbols for the following elements?sulphur, fluorine, titanium, potassium, zinc

Question 50

What are the names of the elements with the following symbols?
Cr, Na, Cl, Be, He

Question 51

What are the names of the elements with the following symbols?
Mn, Mg, Md, Rn, Ra

Question 52

Write formulas of the compounds whose molecular pictures are shown below (unlabelled atoms are carbon).

Question 53

Determine the formula of a compound whose molecules each contain two atoms of carbon, two atoms of oxygen and six atoms of hydrogen.

Question 54

Name three macroscopic properties of orange juice.

Question 55

Plastics are one class of a type of very large molecules called polymers. They are built from smaller building blocks, such as propene. Propene has three carbon atoms and six hydrogen atoms. What is its chemical formula?

Question 56

What are two microscopic properties of a substance?

Question 57

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-The drive to San Francisco from Los Angeles along the coastal route is 450 miles. What is the distance from Los Angeles to San Francisco expressed in SI units using scientific notation?

Question 58

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-What is the volume in SI units of a swimming pool that is 4.5 feet deep by 5 yards wide and 25 yards long?

Question 59

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-You fill your car up in Jamaica and it takes 42.3 L of gasoline. How many gallons is this amount?

Question 60

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-Gold has a density of 19.282 g/cm³. What is the mass (in kg) of a sphere of solid gold with a radius of 6.0 cm? (The volume of a sphere is V = EQ \F(4,3) πr³ where r is the radius.)

Question 61

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-What is the temperature of liquid nitrogen in ˚F, if the nitrogen is currently at -195.8 ˚C?

Question 62

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-A flask with a mass of 160.342 g is filled with 22° C water. The mass of the flask filled with water is found to be 310.5 g. Given that the density of water at 22°C is 0.99780 g/cm³, what is the volume of the flask?

Question 63

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-Fill in the missing quantity:

Question 64

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-When you fill up your car in a country in Europe, your credit card is charged $25.45 for 32.3 L of gasoline. What is the price of gasoline in dollars per gallon?

Question 65

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-Rhodium metal recently was selling for $105.15 per gram. What is the price for a pound of rhodium metal in dollars?

Question 66

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-It has been said that 3.0 kg of plutonium is enough to make an atomic bomb. If you were working security at an airport, just how large of a metallic object would you be looking for? That is, determine the diameter (in cm) of a sphere of plutonium that has a mass of 3.0 kg. (the density of plutonium is 19.84 g/cm³)

Question 67

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-You are asked to administer 4.9 g of an injectable solution which contains 0.23 % of a lifesaving drug by mass. The syringe has graduations of 0.1 mL. If the density of the solution is 1.13 g/mL, how many mL should you inject?

Question 68

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-Ethyl ether has a density of 0.7138 g/ml. How many litres will be needed to obtain 500 grams of ethyl ether for a reaction?

Question 69

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-The density of mercury is 13.6 g/ml and the density of water is 1.00 g/ml. How many meters high would a column of water need to be, to be equal in mass to a column of mercury 750 mm high? (assume the columns of liquid have the same diameter)

Question 70

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-What is the difference in mass between 1.000 x 10¹⁵ protons and the same number of neutrons? What is the electrical charge (in coulombs) carried by this number of protons?

Question 71

Use the following information for Questions
3.785 L = 1 gallon; 2.2 lbs = 1 kg; V = EQ \F(4,3) πr^3; 1 in = 2.54 cm; 1 mile = 1.609 km; 12 in = 1 ft; 1 yard = 3 ft; 1 gal = 3.785 L; ˚C = 5/9 (˚F - 32)
‪
-What is the mass of 1.000 x 10¹⁵ electrons? What is the electrical charge (in coulombs) carried by this number of electrons?

Question 72

Use the following information for Questions .
1 mole = 6.022 x10²³ particles
-Which would have a greater mass: 1.25 mole sample of lead or 11.25 mole sample of aluminum?

Question 73

Use the following information for Questions .
1 mole = 6.022 x10²³ particles
-Which would have a greater mass: a 1.75 mole sample of tin or a 5.25 mole sample of aluminum?

Question 74

Use the following information for Questions .
1 mole = 6.022 x10²³ particles
-Which would have a greater mass: a 2.37 mole sample of potassium or a 3.72 mole sample of magnesium?

Question 75

Use the following information for Questions .
1 mole = 6.022 x10²³ particles
-Naturally occurring platinum has several different isotopes, ¹⁹⁰Pt (0.0127%; 189.960 amu); ¹⁹²Pt (0.78 %; 191.9614 amu); ¹⁹⁴Pt (32.9%; 193.9628 amu), ¹⁹⁵Pt (33.8 %; 194.9648 amu); ¹⁹⁶Pt (25.3 %; 195.9650 amu) and ¹⁹⁸Pt (7.21 %; 197.9675 amu). What is the molar mass of naturally occurring platinum?

Question 76

Use the following information for Questions .
1 mole = 6.022 x10²³ particles
-The density of a particular 300 cm³ graphite sample is 2.16 g cm^-3; how many atoms are contained in the sample?

Question 77

Use the following information for Questions .
1 mole = 6.022 x10²³ particles
-What volume is occupied by an iron sample containing 7.2 x 10²⁵ atoms if the density of the sample is 7.87 g cm³?

Question 78

Calculate the number of moles of carbon atoms and moles of sulphur atoms in 50.0 g of CS₂.

Question 79

Draw a ball and stick model of 1,6-hexanediamine, a starting material for nylon. The line structure is shown below:

Question 80

Determine the molecular formula and draw the line structure for 2-bromobutane.