AnswersWA-Chemistry ACumulative Exam

Cumulative Exam — Cumulative exam Answers

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1
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Which type of reaction is C12H22O11 → 12C + 11H2O?

A
synthesis
B
decomposition
C
oxidation
D
combustion
2
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A sample of ammonia reacts with oxygen as shown.4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)What is the limiting reactant if 4.0 g of NH3 react with 8.0 g of oxygen?

Question illustration
A
O2 because it produces only 0.20 mol of NO.
B
NH3 because it produces only 0.20 mol of NO.
C
O2 because it produces two times less NO than NH3.
D
NH3 because it produces three times more NO than O2.
3

The boiling points of different substances are given in the table below.SubstanceBoiling point (°C)Acetic acid118.1Benzene80.2Chloroform61.2Water100.0Which substance most likely has the strongest intermolecular forces?

A
acetic acid
B
benzene
C
chloroform
D
water
4

Two students are given two different size blocks of the same substance and are instructed to determine the properties of the substance. Which statement describes a property that will be the same for both students?

A
length because it is an extensive property
B
mass because it is an extensive property
C
boiling point because it is an intensive property
D
volume because it is an intensive property
5

Which can be categorized as a use of plasma in technology?

A
taking pictures of solar flares
B
observing the aurora borealis
C
making fluorescent lights for houses
D
making telescopes to observe distant stars
6

The properties of two elements are listed below.ElementAtomic radius(pm)Ionic radius(pm)First ionization energy(kJ/mol)Electron affinity(kJ/mol)ElectronegativityBr1141951140–3253.0K243152.2418.8–48.40.82Which prediction is supported by the information in the table?

A
K will give up an electron more easily than Br.
B
Both K and Br will have the same pull on electrons.
C
K will have a smaller size in comparison to Br.
D
Both K and Br will produce ions of the same size.
7

Consider the balanced equation. PCl3 + 3H2O H3PO3 + 3HCl What is the percent yield of HCl if 42.0 g of HCl are produced from the reaction of 62.0 g of PCl3?Use .

Question illustration
A
28.4%
B
72.8%
C
85.0%
D
93.5%
8

In the molecules below, areas that have a partial negative charge are pink and areas that have a partial positive charge are blue. The attractive force between these two molecules has most likely been produced by

Question illustration
A
covalent bonds.
B
dipole-dipole interactions.
C
dipole-induced dipole interactions.
D
London dispersion forces.
9

Which statement best compares the energy involved in melting with the energy involved in boiling for a given liquid?

A
Energy is removed from the particles in each change, but more energy is removed in melting than in boiling because the attractions are weaker.
B
Energy is removed from the particles in each change, but more energy is removed in boiling than in melting because the attractions are weaker.
C
Energy is added to the particles in each change, but boiling requires more energy than melting because the attractions must be completely overcome.
D
Energy is added to the particles in each change, but melting requires more energy than boiling because the attractions must be completely overcome.
10

An element has five valence electrons available for bonding. This element is most likely which of the following?

A
boron
B
phosphorus
C
tin
D
tellurium
11

Which statement is true about crystal lattice energy?

A
It increases as the size of the ions increases.
B
It increases as the charge on the ions decreases.
C
It is the energy that ions absorb when they form a crystal.
D
It is a measure of the strength of the bonds between ions.
12

Consider the word equation.calcium hydroxide + hydrochloric acid calcium chloride + waterWhich is the corresponding formula equation?

Question illustration
A
Upper C a upper C l subscript 2 right arrow upper C a (s) plus upper C l subscript 2 (g).
Option A
B
Upper C a upper O (s) plus upper H subscript 2 upper O (l) right arrow upper C a (upper O upper H) subscript 2 (a q).
Option B
C
Upper N a upper O upper H (a q) plus 2 upper H upper C l (a q) right arrow upper N a upper C l (a q) plus 2 upper H subscript 2 upper O (l).
Option C
D
Upper C a (upper O H) subscript 2 (s) plus 2 upper H upper C l (l) right arrow upper C a upper C l subscript 2 (a q) plus 2 upper H subscript 2 upper O (l).
Option D
13

Which is a component of John Dalton’s atomic theory?

A
The ratio of atoms in a compound is fixed.
B
The atoms of different elements are the same.
C
An atom is a small particle of matter that can be broken down.
D
A reaction can create or destroy atoms as well as rearrange them.
14

Which diagram shows electrons violating the Pauli exclusion principle?

A
A box contains an up arrow.
Option A
B
A box contains an up and a down arrow.
Option B
C
A box contains an up and a down arrow.
Option C
D
A box contains an up and a down arrow.
Option D
15

The volume of a fixed amount of gas is doubled, and the absolute temperature is doubled. According to the ideal gas law, how has the pressure of the gas changed?

A
It has increased to two times its original value.
B
It has increased to four times its original value.
C
It has decreased to one-half its original value.
D
It has stayed the same.
16

A gas in a rigid container at 25°C has a pressure of 0.96 atm. A change in temperature causes the pressure to increase to 1.25 atm. What is the new temperature of the gas?Use .

Question illustration
A
–44.2°C
B
32.6°C
C
115°C
D
388°C
17

Consider the unbalanced equation for the oxidation of aluminum._Al + _O2 _Al2O3Which sequence of coefficients should be placed in the blanks to balance this equation?

Question illustration
A
2, 3, 1
B
1, 3, 2
C
4, 3, 2
D
3, 2, 3
18

The chemical equation below shows the combustion of methane (CH4).CH4 + 2O2 CO2 + 2H2OThe molar mass of oxygen gas (O2) is 32.00 g/mol. The molar mass of carbon dioxide (CO2) is 44.01 g/mol. What mass of CO2, in grams, will form when 8.94 g O2 completely react?

Question illustration
A
3.25 grams
B
6.15 grams
C
13.0 grams
D
53.0 grams
19

When chemists convert ethene (C2H2) to ethanol (CH3CH2OH), they have a mixture of the two gaseous substances. Why do chemists then lower the temperature of the mixture?

A
to collect liquid ethene and leave ethanol as a gas because ethene has stronger dipole-dipole forces
B
to collect liquid ethene and leave ethanol as a gas because ethanol has stronger London dispersion forces
C
to collect liquid ethanol and leave ethene as a gas because ethanol has hydrogen bonds
D
to collect liquid ethanol and leave ethene as a gas because ethene has stronger London dispersion forces
20

A single atom of an element has 21 neutrons, 20 electrons, and 20 protons. Which element is it?

A
K
B
Zr
C
Ca
D
Sc

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