CHEM 105 - General Chemistry 1 (Fall 2015)

Question 1

Question

Energy is the [blank_start]capacity[blank_end] to do [blank_start]work[blank_end].

Answer

capacity
work

Question 2

Question

Work is the result of a [blank_start]force[blank_end] acting through a [blank_start]distance[blank_end].

Answer

force
distance

Question 3

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What are the two primary methods through which objects or sets of objects exchange energy?

Answer

heat and mass
heat and work
motion and heat
attraction and work

Question 4

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The energy associated with the motion of an object is its [blank_start]kinetic[blank_end] energy.

Answer

kinetic

Question 5

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The energy associated with the position or composition of an object is its [blank_start]potential[blank_end] energy.

Answer

potential

Question 6

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[blank_start]Chemical[blank_end] energy, a form of potential energy, is associated with the relative positions of electrons and nuclei in atoms and molecules.

Answer

Chemical

Question 7

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The energy associated with the temperature of an object is its [blank_start]thermal[blank_end] energy.

Answer

thermal

Question 8

Question

The law of conservation of energy, or the first law of thermodynamics, states that energy can be neither created nor destroyed. This means that the total energy of the universe is constant.

Answer

True
False

Question 9

Question

The SI unit of energy is the joule (J). Which of the following is true about this unit?

Answer

1 J = 1 g * m^2 / s^2
1 J = 1 kg * m^2 / s^2
1 J = 1 kg * m / s^2
1 J = 1 kg * m^2 / h^2
1 J = 1 kg * m^2 / s

Question 10

Question

Besides joules, a calorie is another commonly used energy unit: 1 cal = [blank_start]4.184[blank_end] J 1 Cal = 1 [blank_start]kcal[blank_end] = [blank_start]1000[blank_end] cal

Answer

kcal
1000
4.184

Question 11

Question

Besides joules, a kilowatt-hour is another unit of energy commonly used for electricity bills: 1 kWh = [blank_start]3.60[blank_end] * [blank_start]10^6[blank_end] J

Answer

3.60
10^6

Question 12

Question

The internal energy (E) of a system is the sum of the kinetic and potential energies of all of the particles that compose the system.

Answer

True
False

Question 13

Question

Internal energy is a state function, which means that its value depends only on the state of the system, not on how the system arrived at that state.

Answer

True
False

Question 14

Question

Which of the following is true about a system's energy?

Answer

ΔE(sys) = -ΔE(surr)
2ΔE(sys) = -ΔE(surr)
ΔE(sys) = ΔE(surr)
ΔE(sys) = -3ΔE(surr)
-ΔE(sys) = -ΔE(surr)

Question 15

Question

If the reactants have a higher internal energy than the products, ΔE(sys) is [blank_start]negative[blank_end] and energy flows [blank_start]out of[blank_end] the system into the surroundings. If the reactants have a lower internal energy than the products, ΔE(sys) is [blank_start]positive[blank_end] and energy flows [blank_start]into[blank_end] the system from the surroundings.

Answer

negative
out of
positive
into

Question 16

Question

Which of the following represents heat?

Answer

Question 17

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Which of the following represents change in internal energy for a given system?

Answer

Question 18

Question

ΔE = [blank_start]q[blank_end] + [blank_start]w[blank_end]

Answer

Question 19

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What is the difference between heat and thermal energy?

Answer

Temperature is a measure of the thermal energy within a sample of matter, whereas heat is the transfer of thermal energy.
Heat is a measure of the thermal energy within a sample of matter, whereas temperature is the transfer of thermal energy.
Temperature is a measure of the total energy within a sample of matter, whereas heat is a measure of temperature change.
Heat is a measure of the total thermal energy within a sample of matter, whereas temperature is a measure of heat change.

Question 20

Question

The constant of proportionality between q and ΔT is the system’s heat capacity (C), a measure of the system’s ability to absorb thermal energy without undergoing a large change in temperature. C is defined as the quantity of heat required to change a system's temperature by 1 °C: q = [blank_start]C[blank_end] × Δ[blank_start]T[blank_end]

Answer

Question 21

Question

What is the difference between heat capacity and specific heat capacity?

Answer

Heat capacity is the ratio of the amount of energy absorbed to the associated temperature rise, whereas specific heat capacity is the heat capacity of a substance per unit mass.
Specific heat capacity is the ratio of the amount of energy absorbed to the associated temperature rise, whereas heat capacity is the specific heat capacity of a substance per unit mass.
Heat capacity is the ratio of the amount of energy absorbed, whereas specific heat capacity is the difference in heat capacity.

Question 22

Question

Which of the following is true about heat?

Answer

q = m / C(s) × ΔT
q = 2m × C × ΔT
q = m × C(s)
q = m × C(s) × ΔT
q = m × C / ΔT

Question 23

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F = [blank_start]P[blank_end] * [blank_start]A[blank_end]

Answer

Question 24

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w = -[blank_start]P[blank_end]Δ[blank_start]V[blank_end]

Answer

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CHEM 105 - General Chemistry 1 (Fall 2015)

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