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Honors Chemisty > Practice Final Exam > Flashcards

Practice Final Exam Flashcards

1
Q

Which of the following elements of the scientific method is a concise summary of repeated scientific observations?

A

A scientific law.

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2
Q

Which of the following statements is not a part of Dalton’s atomic theory.

A

The number of protons determines the identity of an atom

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3
Q

An intensive property such as density is only relevant to pure substances and homogeneous mixtures, and not to heterogeneous mixtures.

A

false

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4
Q

What distinguishes a mixture from a pure substance?

A

A mixture is a combination of two or more substances that are physically separable, and a pure substance is not physically separable.

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5
Q

Looking at this entry from the periodic table, which of the arrows points to the atomic number?

A

1

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6
Q

Iodine (I), displays reactivity similar to _____.

A

fluorine (F)

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7
Q

What is the coefficient for oxygen in the properly balanced equation for the combustion of propanol in oxygen gas to form carbon dioxide gas and water according to the equation:

A

9

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8
Q

What two conversion factors would be used to determine how many atoms of iron are contained in 10 grams?

A
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9
Q

Ammonia (NH3) is produced industrially using the Haber-Bosch process (1912) which combines nitrogen (N2) and hydrogen (H2) at high temperatures (500°C) and high pressures (200 atm). What is the theoretical yield of ammonia (NH3) that can be produced when a cylinder containing 50.0 kg of nitrogen gas (N2) is reacted with excess hydrogen gas (H2)?

A

60.8 kilograms (3570 moles).

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10
Q

Which of the following represents the net ionic equation of the combination of insoluble of aluminum hydroxide and a solution of hydrobromic acid?

A

Al(OH)3(s) + 3H+(aq) —> Al3+(aq) + 3H2O(l)

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11
Q

30.0 mL of a sulfuric acid solution of unknown molarity is titrated against 27.3 mL of a standardized 0.55 M sodium hydroxide solution. What is the concentration of the sulfuric acid solution? Recall that sulfuric acid is a diprotic acid.

A

0.25 M H2SO4

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12
Q

A balloon containing 4.28 L of an unknown gas at 1.00 atm and 298 K has a mass of 16.90 g. The empty balloon has a mass of 2.24 g. What is the molar mass of the gas in the balloon?

A

83.8 g/mol

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13
Q

Calculate the average speed (root-mean-square speed) of a gas that has a molar mass of 1.73 × 10−2 kg / mol at a temperature of 39°C. The value for the gas constant, R, is 8.314 J / mol K. Also, remember that 1 J = 1 kg m2/s2, so 1 J / kg = 1 m2/s2.

A

671 m / s

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14
Q

In the field of thermodynamics, what are the surroundings?

A

everything other than the system

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15
Q

A coffee cup (or constant pressure) calorimeter contains 108.0 g of water at an initial temperature of 25.0°C. 118.7 g of tin metal at a temperature of 100°C is added. The final temperature in the calorimeter is 29.2°C. What is the molar heat capacity of the tin? The molar heat capacity of water is 75.4 J / (mol•°C). Assume that the heat capacity of the coffee cup is negligible.

A

26.8 J / (mol•°C)

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16
Q

Only the number of valence electrons has an influence on the chemical properties of an element.

A

false

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17
Q

As you move from the left to the right across the periodic table, which of the following is the trend?

A

Increasing ionization energy

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18
Q

Which of the following compounds is not expected to form:

A

NaCO3

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19
Q

The electron configuration of argon is 1s22s22p63s23p6.

How many valence electrons does argon have?

A

8

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20
Q

Which of the following is the correct Lewis dot structure of the ethoxide anion, [CH3CH2O]−?

A
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21
Q

What are the oxidation numbers for magnesium and oxygen (in that order) in the MgO molecule?

A

+2, −2

22
Q

For London dispersion forces to be present, the molecule must have a permanent dipole moment.

A

false

23
Q

Which of the following statements about a saturated solution is not true?

A

In a saturated solution, the solute atoms and molecules no longer change states (between dissolved and undissolved solute) because equilibrium exists.

24
Q

When making home-made ice cream, table salt, sodium chloride, is mixed with ice to lower the temperature. Suppose 500 grams of salt are mixed with 8.0 liters of water to make a solution. What is the freezing point of this solution?

A

−3.98°C

25
Q

Ink is composed of a solid dispersed in a liquid. Therefore, ink is a(n) _____.

A

sol

26
Q

Using the following data for the reaction 2NO2(g) + F2(g) → 2FNO2(g), what are the values of m, n, and k in the rate law rate = k[ NO2 ]m [ F2 ]n?

A

m = 1, n = 1, k = 24 M −1 • s−1

27
Q

The data below is for a reaction A → B + C. True or false: this reaction is second-order in A.

A

true

28
Q

The Arhenius Equation can be rearranged into the form of an equation of a straight line. What parameters are plotted in order to determine the Ea of a reaction by graphical method?

A

Plot ln of k versus the 1/T

29
Q

The accepted mechanism for the reaction of methane (CH4) and chlorine (Cl2) to produce chloromethane (CH3Cl) is:

Based on this mechanism, what is the rate law for this reaction?

A

rate = k[Cl2]

30
Q

______ is an enzyme in blood which catalyzes the same reaction as iodide ion and manganese(IV) oxide.

A

catalase

31
Q

If the value of the equilibrium constant with regard to pressure (Kp ) is found to be 1.5 at 15°C, what is the value of the eqilibrium constant with regard to concentration?
(R = 0.0821 L • atm / (mol • K))

N2(g) + 2O2(g) N2O4(g)

A

8.4 × 102

32
Q

A strong acid has a weak conjugate base because:

A

The conjugate base is a species that gave up a proton easily (as a strong acid), it is therefore going to be a poor proton acceptor.

33
Q

What is the percent dissociation of a 0.20 M solution of the weak base methylamine? (NH2CH3 )?
(Kb = 4.4 × 10−4 )

A

4.7

34
Q
A

Reaction C is the reverse reaction of the autoionization of water. Koverall = Ka(1 / Kw ).

35
Q

You add 0.01 moles of normally insoluble silver chloride (AgCl) to 1 L of 0.800 M ammonia (NH3). The following reaction occurs: Ag+(aq) + 2NH3(aq) Ag(NH3)2+(aq) Kf = 1.7 * 10^7 What is the equilibrium concentration of silver ion (Ag+)?

A

9.2 x 10–10

36
Q

The greater the difference in electronegativity between two atoms, the more polarized the bond, and the more likely the bond will break heterolytically.

A

true

37
Q

Given the following reaction: Ch3NH2(aq) + H2O(l) CH3NH3+(aq) + OH-(aq)

Which species is the conjugate acid of methylamine?

A

CH3NH3+

38
Q

A Brønsted-Lowry acid is a molecule that can donate an electron pair.

A

false

39
Q

Which of the following statements about the leaving group is TRUE?

A

The weaker the base, the better it is as a leaving group.

40
Q

Which of the following defines the entropy change (ΔS) for a system at equilibrium?

A

ΔS = q/T

41
Q

The reaction between hydrogen gas and oxygen gas to produce water is very exothermic, and equilibrium lies very far to the right. Which of the following describes ΔG for this reaction at equilibrium?

A

ΔG = 0 kJ/mol

42
Q

Which of the following is the properly balanced equation for the net ionic equation below in acidic solution?

MnO4-(aq) + CN-(aq) —> MnO2(aq) + OCN-(aq)

A

2H+(aq) + 2MnO4-(aq) +3CN-(aq) —> 2MnO2(aq) + H2O(l) + 3OCN-(aq)

43
Q

What is the pH of a solution used in the following galvanic cell with a potential (Ecell ) of −0.365 V at 25°C?

Ni(s)|Ni2+ (0.1M)||H + (?)|H2(1 atm)

2H+(aq) + Ni(s) H2(g) + Ni2+(aq)
reduction potentials: E degree
H+ + e- 1/2H2 0.000 V
Ni2+ + 2e- Ni -0.230 V

R • T / F = 0.0592 at 25°C

A

10.5

44
Q

Which of the following is a disadvantage of a lead-acid storage battery?

A

it has a low energy-to-mass ratio

45
Q

Galvanized iron is iron with a layer of zinc coated on it. How does the galvanization protect the iron from corrosion?

A

Zinc primarily acts as a sacrificial anode, but is also capable of acting as a passivation agent.

46
Q

In order for electroplating to work, the reduction potential of the metal must be ___________ the reduction potential for water.

A

higher than

47
Q

A semiconductor is able to conduct a current:

A

in both the conduction band and the valence band.

48
Q

How are the alkali metals generally isolated?

A

Reduction of the chloride salt by chemical or electrical means

49
Q

Which of the following is not a part of DNA?

A

Ribose

50
Q

Look at the two propanol molecules.

Which statement about these molecules is not correct?

A

In alcohol molecules with three or fewer carbons, the location of the OH group must be specified.

Honors Chemisty (145 decks)

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