Free Printable Chemistry Spring 21' Cumulative Final Exam Review

Worksheets

Chemistry Spring 21' Cumulative Final Exam Review

Total questions: 112

Worksheet time: 28hrs 0mins

Name

Class

Date

-32.1 kJ

-31.1 kJ

-38.1 kJ

31.8 kJ

Calculate the enthalpy of reaction (ΔH).

4CO_{2 (g)} + 6H₂O _(g) → 2C₂H_{6 (g)} + 7O_{2 (g)}

ΔH_f^o [CO_2(g)] = -393.5 kJ

ΔH_f^o[H₂O_(g)] = -241.8 kJ

ΔH_f^o [C₂H_6(g)] = -84.7 kJ

ΔH_f^o [O_2(g)] = 0 kJ

550.6 kJ/mol

2855.4 kJ/mol

-550.6 kJ/mol

-3194.2 kJ/mol

The specific heat of water is 4.18 J/g°C.

If 980. J of energy is added to 6.20 g of water at 18.0 °C, what is the final temperature of the water?

37.8 °C

-19.8 °C

19.8 °C

55.8 °C

The standard enthalpy of reaction (ΔH) for the reaction below is -65.2 kJ.

Determine the enthalpy of formation for Calcium Hydroxide (Ca(OH)₂ (s)

CaO_(s) + H₂O _(l) → Ca(OH)_2(s)

ΔH_f^o [CaO(s)] = -635.6 kJ

ΔH_f^o[H₂O_(l)] = -285.8 kJ

-966.6 kJ

-986.6 kJ

986.6 kJ

-968.6 kJ

$q=m\ x\ cp\ x\ \Delta T$

The specific heat equation is shown above, what does cp stand for?

the heat released or absorbed by a system

specific heat of a substance

mass of a substance

change in temperature

A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample? (show your work)

25g

30g

20g

50g

What unit do you use to measure Thermal Energy?

J/Kg ºC

ºC

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams of copper?

12.82 °C

24.12°C

351 °C

$q=m\ x\ cp\ x\ \Delta T$

The specific heat equation is shown above, what does q stand for?

the heat released or absorbed by a system

specific heat of a substance

mass of a substance

change in temperature

10.

$q=m\ x\ cp\ x\ \Delta T$

The specific heat equation is shown above, what does m stand for?

the heat released or absorbed by a system

specific heat of a substance

mass of a substance

change in temperature

11.

$q=m\ x\ cp\ x\ \Delta T$

The specific heat equation is shown above, what does Delta T stand for?

the heat released or absorbed by a system

specific heat of a substance

mass of a substance

change in temperature

12.

In an endothermic reaction the system is releasing energy.

True

False

Sometimes

13.

In an exothermic reaction, heat is ...

taken in

given out

nothing happens

it gets colder

14.

Methane combusts with oxygen through the following reaction: CH₄+2O₂→CO₂+2H₂O

How many grams of carbon dioxide are produced when 16.0 g of methane and 48.0 g of oxygen gas combust?

Molar mass of CH4 = 16.0 g/mol

Molar mass of O2 = 32.0 g/mol

Molar mass of CO2 = 44.0 g/mol

Choose the closest approximate answer

33 grams

66 grams

64 grams

92 grams

15.

What mass of silver nitrate will react with 5.85 grams of sodium chloride to produce 14.35 grams of silver chloride and 8.5 grams of sodium nitrate?

AgNO₃(aq)+NaCl(aq)→AgCl(s)+NaNO₃(aq)

Molar mass of AgNO3 = 169.87 g/mol

Molar mass of NaCl = 58.44 g/mol

Molar mass of AgCl = 143.32 g/mol

Molar mass of NaNO3= 84.99 g/mol

23.5 grams

21.2 grams

17.0 grams

14.2 grams

16.

Lead nitrate can be decomposed by heating. What is the approximate % yield of the decomposition reaction if 7.4g Pb(NO₃)₂ are heated to give 4.1 g PbO?

2Pb(NO₃)_{2 (s)}→2PbO_(s)+4NO_2(g)+O_2(g)

Molar Masses:

-Pb(NO₃)₂= 331.2 g/mol

-PbO = 223.2 g/mol

82%

44%

56%

67%

17.

For the Balanced Reaction: 3 Mg + 1 Fe₂O₃ → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?

3mol Mg / 2 mol Fe

2 mol Mg/ 3 mol Fe

1 mol Fe/ 2 mol Fe

3 mol MgO / 2 mol Fe

18.

2NaClO₃ (s) → 2NaCl (s) + 3O₂ (g)

12.00 moles of NaClO₃ will produce approximately how many grams of O₂?

Molar Masses:

NaClO₃ = 106.44 g/mol ; O₂ = 32.00 g/mol

256 g of O₂

576 g of O₂

288 g of O₂

384 g of O₂

19.

What is correct equation that should be used to determine how many formula units there are in 0.75 moles of (NH₄)₃PO₄?

20.

2H₂ + O₂ → 2H₂O
How many moles of water can be produced if 8 moles H₂ are used?

4 moles

8 moles

16 moles

2 moles

21.

Cl₂ + 2KBr → Br₂ + 2KCl

Approximately how many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?

Molar Masses:

KCl = 74.55 g/mol ; KBr = 119.00 g/mol

749 g

223 g

479 g

814 g

22.

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

theoretical yield

mole ratio

actual yield

percentage yield

23.

What is the molar mass of NaOH?

40.00 g/mol

38.99 g/mol

23.99 g/mol

57.00 g/mol

24.

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl₂.

Mg + 2HCl --> MgCl₂ + H₂

MgCl2

HCl

25.

How many moles are in 8.30 X 10²³ molecules of H₂O?

1.38 X 10²³ moles H₂O

1.38 moles H₂O

2 moles H₂O

1 mole H₂O

26.

What is the density of ammonia gas (NH₃) in g/L at 0.913 atm and 20° C?

*Choose the closest answer*

*molar mass ammonia= 17.031 g/mol*

64.7 L

.647 g

.647 g/L

6.47 g/L

27.

2CO + O₂−-> 2CO₂

How many liters of carbon monoxide at 25.0^oC and 8.56 mmHg are needed to react with 12.30 L of oxygen gas at STP?

*Molar mass oxygen gas= 32 g/mol

molar mass carbon monoxide= 28.01 g/mol*

3.14 L

318 L

2390 L

200 L

28.

4NH₃+6NO --> 5N₂ + 6H₂O

How many liters of NH₃ at 32.6 ^oC and 4.25 kPa are needed to react completely with 30.0L of NO at STP?

*Choose the closest answer*

*Molar mass nitric oxide= 30.01 g/mol

molar mass ammonia= 17.031 g/mol*

5.27 L

534 L

5.2 L

533.6 L

29.

In the equation PV = nRT, what value of R must be used if the pressure is in atm?

0.08206

62.4

22.4

6.02 X 10²³

30.

In the equation PV = nRT, what value of R must be used if the pressure is in mm Hg?

0.08206

62.36

22.4

6.02 X 10²³

31.

In the equation PV = nRT, what value of R must be used if the pressure is in kPa?

0.08206

62.36

8.314

6.022 X 10²³

32.

Which of the following shows the correct Temperature and Pressure values for a gas at STP?

P= 1.00 atm; T= 273K or 0.00⁰ C

P= 1.00 mmHg; T= 273K or 0.00⁰ C

P= 1.00 kPa; T= 273K or 0.00⁰ C

P= 1.00 atm; T= 273 ⁰ C

33.

A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?

0.78 atm

1.65 atm

1.28 atm

0.61 atm

34.

What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT

14.19 atm

16.53 atm

18.42 atm

22.54 atm

35.

Mg₃N₂ + 3H₂O ––> 3 MgO + 2NH₃

If 10.3 g of magnesium nitride is used, what volume of ammonia gas would be collected at 20˚C and 0.989 atm?

*Molar mass magnesium nitride= 100.95 g/mol

molar mass ammonia= 17.031 g/mol*

6.94 L NH₃

4.96 L NH₃

4.96 g NH₃

4.96 atm NH₃

36.

In a solution, the substance that is dissolved is called the _________________.

colloid

solute

solvent

suspnsion

37.

The process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules is called _________________

solvation

dissolving

plucking

pulling

38.

Water and Kool-Aid are mixed together. Hot water, coffee and sugar are mixed together. Which substance is the solvent in both?

Water

Coffee

Kool-aid

Sugar

39.

This solution would be considered

Unsaturated

Supersaturated

Saturated

Undefined

40.

This graph represents a(n) ___ solution

saturated

supersaturated

unsaturated

undefined

41.

____________________________ is the concentration of a solution expressed as the number of moles of solute dissolved in each liter of solution.

molality

% by mass

molarity

mole fraction

42.

A _______________ solution contains as much solute as can possibly be dissolved under existing conditions of temperature and pressure.

supersaturated

saturated

unsaturated

Chick - Fil -A

43.

The solubility graph below shows the amounts of four substances that will dissolve in 100 grams of water at various water temperatures.

Which substance has 80 grams of solute dissolved in 100 grams of water at 50 C?

Potassium Bromide

Ammonium Chloride

Potassium Chloride

Lithium Hydroxide

44.

Which substance is MOST soluble at 0 ºC?

NaNO₃

NaCl

Ce₂(SO₄)₃

45.

When 50 grams of potassium chloride, KCl, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:

supersaturated

unsaturated

saturated

Not a solution at all

46.

A solution of potassium chlorate, KClO₃, has 20 grams of salt dissolved in 100 grams of water at 70 ºC. Approximately how many more grams of salt can be added until the solution becomes saturated?

10 grams

30 grams

80 grams

60 grams

47.

A solution with a total volume of 1000 ml has 2.0 moles of solute dissolved in it. What is the molarity of the solution?

2.0 M

0.002 M

2000 M

500 M

48.

What is the molarity of a solution containing 40 g NaCl in 2.0 liters of solution?

0.34 M

20 M

0.05 M

80 M

49.

How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide?

50.

How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?

1074 mol

0.069 mol

1.07 mol

62.7 mol

51.

A 0.500 M solution of formic acid is prepared, and its pH is measured to be 2.04. Determine the Ka for formic acid.

Ka = [H+][HCOO-]/[HCOOH]

*Equilibrium values: [HCOOH]=0.491; [H+]/[HCOO-]=9.12 x10^-3*

9.12 x 10 ^-3

9.12 x 10 ³

1.7 x 10^-4

1.7 x 10⁴

52.

A solution contains 0.04 M of a weak acid. Calculate the pH of the solution knowing that the K_a for the acid is 1.6 x 10^-7

It is not possible to solve if the identity of the acid is not known

4.1

4.9

Because the Ka is very small, the pH is close to neutral (about 6)

53.

What is the pOH of a solution with [H⁺] = 1.24 x 10 ^-2?

1.91

1.61

12.09

12.39

54.

Which is the correct formula for writing an base ionization constant expression for the following equation involving ammonia:

NH3 + H2O →NH4⁺ (aq) + OH^-(aq)

$Kb=\frac{\left[NH4\right]}{\left[NH3\right]}$

$Kb=\frac{\left[NH4+\right]\left[OH-\right]}{\left[NH3\right]}$

$Kb=\frac{\left[NH3+\right]\left[OH-\right]}{\left[NH4\right]}$

$Kb=\frac{\left[NH3\right]}{\left[NH4+\right]\left[OH-\right]}$

55.

Which is the correct Acid Ionization constant expression for the following reaction involving Hydrofluoric Acid:

HF----> H+ + F-

$Ka=\frac{\left[H+\right]\left[F-\right]}{\left[HF\right]}$

$Ka=\frac{\left[H+\right]\left[A-\right]}{\left[HF\right]}$

$Ka=\frac{\left[F+\right]\left[H-\right]}{\left[HF\right]}$

$Ka=\frac{\left[HF\right]}{\left[H+\right]\left[F-\right]}$

56.

A solution of KOH is 2.5 x 10^-5M. What is the [H⁺] concentration? (Hint: Find pOH, then pH, then [H⁺].)

4.60

9.40

3.98 x 10^-10

1.0 x 10^-4.60

57.

If a solution has a pOH of 3.7 the [OH-] of the solution is

5.0 x 10^-11

2.0 x 10^-4

10.3

58.

If [OH-] = 1 x 10^-4 M, what is the pH of the solution?

-4

-10

59.

The [OH-] concentration of a solution = 3.0 × 10⁻⁵ M; calculate [H+] and determine if the solution is acidic or basic.

*Use K_w= 1.0 x10^-14 *

[H+] = 3.3 x 10 ¹⁰; the solution is basic

[H+] = 3.3 x 10 ^-10; the solution is acidic

[H+] = 3.3 x 10 ^-10; the solution is basic

[H+] = 3.3 x 10 ¹⁰; the solution is acidic

60.

0.750 M solution of the weak base ethylamine (C2H5NH2) has a pOH of 1.69, what is Kb?

Kb = [C2H5NH3+][OH-]/[C2H5NH2]

*Equilibrium values: [C2H5NH2]=0.730; [C2H5NH3+]/[OH-]=2.04 x 10^-4*

5.7 x 10 ^-4

5.7 x 10 ⁴

4.16 x 10^-4

4.16 x 10 ⁴

61.

What is the pH of a 0.053 M solution of potassium hydroxide

6.91

12.72

7.33

1.28

62.

A certain solution has a pH of 1.93. Calculate its [H⁺] and [OH⁻].

[H⁺] = 1.2 x 10 ^-2 M ; [OH⁻] = 8.3 x 10 ^-13 M

[H⁺] = 1.2 x 10 ² M ; [OH⁻] = 8.3 x 10 ¹³ M

[H⁺] = 8.3 x 10 ¹³ M ; [OH⁻] = 1.2 x 10 ² M

[H⁺] = 8.3 x 10 ^-13 M ; [OH⁻] = 1.2 x 10 ^-2 M

63.

What is the [OH^-] of a solution whose pH = 5.43 ?

*K_w = [H+][OH-] or 1.0 x 10^-14*

8.57

2.69 x 10^-9 M

3.72 x 10^-6 M

269153

64.

What is the equation for calculating pH?

pH = [H⁺]

pH = log [H⁺]

pH = -log[OH^-]

pH = -log [H⁺]

65.

What is the [OH-] if the pH is 4.9?

4.9 x 10^-10 M

1.0 x 10^-4 M

1.25 x 10^-5M

7.94 x 10^-10 M

66.

What is the [OH-] if the [H+] is 1.0 x 10^-3M?

1.0 x 10^-3 M

1.0 x 10^-14 M

6.02 x 10^-23 M

1.0 x 10^-11 M

67.

If the [OH^-] of a solution is 2.7 x 10^-4 M, the pOH of the solution is

10.44

1.00

3.57

-4.43

68.

If the pH of a solution is 4.0, what is the pOH?

4.0

10.0

1.0 x 10 ^-4

cannot be determined from the information

69.

Sodium hydroxide (NaOH) is a strong base. Find the pH of a solution prepared by dissolving 1.0 g of NaOH into enough water to make 1.0 L of solution.

*The molar mass of NaOH = 40.00 g/mol; K_w = [H+][OH-] or 1.0 x 10^-14;Molarity = mol solute / L of Solution*

124.0

12.40

1.240

70.

If a solution has a [H⁺] of 9.3x10^-11, what is the pH?

10.0

4.0

3.5

8.2

71.

Hydrochloric acid (HCl) is a strong acid, meaning that it is essentially 100% ionized in solution. What are the values of [H+] and [OH−] in a 2.0 × 10⁻³ M solution of HCl?

*use K_w = 1.0 × 10⁻¹⁴ *

[H+]= 2.0 × 10⁻³ M; [OH−]=5.0 × 10⁻¹²M

[H+]= 2.0 × 10³ M; [OH−]=5.0 × 10⁻¹²M

[H+]= 2.0 × 10^-3 M; [OH−]=5.0 × 10¹²M

[H+]=5.0 × 10⁻¹²M ; [OH−]= 2.0 × 10⁻³ M

72.

The Kw at room temperature (25 degrees C) is equal to 1.0 x 10-14. It can also be defined as:

the pH and pOH of a solution

the product of the hydronium ion and the hydroxide ion concentrations

-log [hydronium ion]

antilog -pH

73.

What is the concentration of H⁺ in a solution with a pH of 3?

1.0 x 10^-3

3.0 M

10.3 M

10³ M

74.

Which of the following is the hydrogen ion concentration of an acid?

9.2 x 10^-14

2.4 x 10^-7

1.0 x 10^-8

5.7 x 10^-11

75.

Which of the following is the [H⁺] concentration of a base?

9.2 x 10^-3

8.3 x 10^-6

3.4 x 10^-9

1.7 x 10^-7

76.

The pH of a solution is 8.43. What is the hydroxide ion OH^- concentration?

3.7 x 10^-9 M

2.7 x 10^-6 M

antilog (-pH)

1.0 x 10^-14/-pH

77.

The [H+] concentration of a solution = 4.0 × 10⁻⁸ M; calculate [OH-] and determine if the solution is acid or basic.

*Use K_w= 1.0 x10^-14 *

[OH-] = 2.5 x 10 ¹⁴; the solution is basic

[OH-] = 2.5 x 10 ^-7; the solution is acidic

[OH-] = 2.5 x 10 ^-7; the solution is basic

[OH-] = 2.5 x 10 ^-14; the solution is acidic

78.

What is the concentration of hydroxide ions in a 2.0 M HCl solution?

5.0 E-15 M OH^-

2.0 M OH^-

2.0/1.0 E-14 M OH^-

antilog (-2.0)

79.

NaOH is:

an Arrhenius base

an Arrhenius acid

neither an acid nor a base

both an acid and a base

80.

In this reaction...
CH₃NH₂ + H₂O --> CH₃NH₃⁺ + OH^-CH₃NH₂ can be classified as which of the following? (HINT...follow the H⁺!!!)

A Brønsted-Lowry base

A Brønsted-Lowry acid

A Lewis acid

An Arrhenius acid

81.

In the reaction HCl + H₂O --> H₃O⁺ + Cl^-, what is the conjugate acid?

HCl

H₂O

H₃O⁺

Cl^-

82.

The Acid-Base classification system that defined a __________ is any compound that can donate a proton (an H⁺ ion) to an appropriate acceptor. A _________ is a compound that can remove (or accept) a proton.

Bronsted-Lowry acid; Bronsted-Lowry Base

Arrhenius acid; Arrhenius-base

Lewis acid; Lewis Base

Monoprotic and Polyprotic Acids

83.

The Acid-Base classification system that defined any chemical species that accepts a pair of electrons as a _______, and a _________ is a chemical species that donates a pair of electrons.

Bronsted-Lowry Acid; Bronsted-Lowry Base

Arrhenius acid; Arrhenius base

Lewis acid; Lewis base

Monoprotic and Polyprotic Acids

84.

The Acid-Base classification system that defined acids as those that release H⁺ and bases as release OH^- is known as ________.

Bronsted-Lowry

Arrhenius acid-base

Lewis acid-base

Monoprotic and Polyprotic Acids

85.

Why does an atom undergo beta decay?

It has too many electrons.

It has an atomic number greater than 83

It has more neutrons than protons

It has more protons than neutrons

86.

What type of nuclear equation is this?

fusion

fission

alpha

beta

87.

In fission, a neutron is often used to start the reaction and it is also a product of the reaction. This is called a ____

neutron emission

nuclear fusion

domino effect

chain reaction

88.

In a neutral atom, the number of protons always equals

the number of neutrons.

the number of electrons.

the mass number.

the average atomic mass.

89.

What do these symbols represent?

alpha particle

beta particle

neutron

gamma ray

90.

What fuel does the US typically use in fission reactors?

Hydrogen

Carbon

Uranium

Plutonium

91.

This is the symbol for a(n)

alpha particle

beta particle

gamma particle

92.

²³⁶₉₂U

²³⁶₉₃U

²³⁴₉₂Np

²³⁴₉₃Np

93.

What is the missing isotope that will balance the following nuclear equation?
⁹₄Be + ¹₁H → _____ + ⁴₂He

¹⁰₅B

¹⁰₅Ne

⁶₃Li

⁶₃C

94.

Barium-122 has a half-life of 2 minutes. A fresh sample weighing 80 g was obtained. If it takes 10 minutes to set up an experiment using barium-122, how much barium-122 will be left when the experiment begins?

0.25g

2.5g

25g

80g

95.

What is the half-life of an isotope if after 20.0 days you have 4.0 grams remaining of a 64.0 grams sample?

1.25 days

5.0 days

0.000305 days

4.25 days

96.

What type of decay is this?
⁷⁵₃₄Se + ⁰_-1e --> ⁷⁵₃₃As

Electron Capture

Positron Emission

Alpha Decay

Beta Decay

97.

Scientist involved with discovery of radioactivity.

Albert Einstein

Ernest Rutherford

Marie Curie

Isaac Newton

98.

Which process involves the joining of small nuclei?

Beta decay

Alpha decay

Nuclear fission

Nuclear fusion

99.

What is the equation for the positron emission by oxygen-16?

¹⁶₈O + ⁰₊₁e --> ¹⁶₉F

¹⁶₈O --> ⁴₂He + ¹²₆C

¹⁶₈O --> ⁰_-1e + ¹⁶₉F

¹⁶₈O --> ⁰₊₁e + ¹⁶₇N

100.

What is the symbol for an alpha particle?

⁴₂He

⁰_-1e

⁰₊₁e

¹₀n

101.

If Thorium-234 undergoes a beta decay, What element will be left in its place?

Actinium-234

Thorium-233

Protactinium-234

Radium-230

102.

The half life of Thorium-234 is 24 days. What fraction of the element remains after 96 days

1/2

1/4

1/8

1/16

103.

Balance the following equation:
¹⁴₆C --> ⁰_-1e + ________

¹⁴₅B

¹⁴₆C

¹⁴₇N

⁴₂He

104.

The technetium-99 isotope has a half-life of 6.0 hours. If 100.0 mg were injected into a patient how much remains after 18 hours?

33.0 mg

12.5 mg

.33 mg

15.8 mg

105.

⁴₂He

⁰_-1e

⁰₀Y

¹⁷₈O

106.

Complete the nuclear reaction

⁴₂He

⁰_-1e

⁰₀γ

¹⁷₈O

107.

What happens to the atomic number during alpha decay?

The atomic number decreases by 4

The atomic number increases by 1

The atomic number decreases by 2.

The atomic number stays the same.

108.

Which process involves the splitting of large nuclei?

Beta decay

Alpha decay

Nuclear fission

Nuclear fusion

109.

What does it mean when an element is radioactive?

atom emits radiation

nuclei are unstable due to uneven proton to neutron ratio

nuclei changes to become stable

all of the above

110.

In the symbol ¹⁶₇N what the 7 stand for?

Mass number

Atomic number

Atomic mass

Number of neutrons

111.

The time taken for half of an amount of radioactive atoms to decay.

Nuclear fusion

Full-life

Dead time

Half-life

112.

Alpha particles have a _____ charge.

-1

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Chemistry Spring 21' Cumulative Final Exam Review

Total questions: 112

Worksheet time: 28hrs 0mins

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