Calorimetry (AKA Heat Problems or Thermochemistry) Flashcards

1
Q

Heat being absorbed is an example of an_______ process.

A

endothermic

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2
Q

Heat being released is an example of an ________ process

A

exothermic

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3
Q

H2O (l) –> H2O (s) is an _______ process and the word Heat would be put on the _______ side of the arrow.

A

exothermic; right

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4
Q

What is sublimation? Give 2 examples of substances that undergo it.

A

Solid changing to gas without turning into a liquid first. ; dry ice (CO2) or Iodine (s)

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5
Q

What is fusion and what equation do you use for it?

A

melting; q= mHf

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6
Q

Why is there no temperature change when a solid becomes a liquid at the melting point?

A

The heat energy is being absorbed in order to change phase and increase the PE. The temperature won’t go up until all the molecules have changed phase.

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7
Q

What is the technical definition of temperature in terms of molecular movement?

A

Temperature is defined as the average kinetic energy of molecules.

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8
Q

On a phase change diagram, when does KE go up?

A

During a slant of the line (when the temperature is changing)

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9
Q

What phase of matter has the most PE?

A

Gas has the most PE.

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10
Q

What does entropy refer to? What phase of matter has the most entropy?

A

Randomness or disorder of a system (or substance); Gases have the most entropy.

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11
Q

When would you use the equation: q= mcDeltaT?

A

When you want to know how much heat is absorbed or released by a substance that undergoes a change in temperature..

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12
Q

What is the unit for specific heat capacity?

A

J/gC

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13
Q

What is the opposite of vaporization? What phase change occurs?

A

Condensation; Gas –> liquid

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14
Q

At what temperature does vaporization occur?

A

The boiling point.

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15
Q

What is the difference between evaporation and vaporization?

A

evaporation can occur at room temperature; vaporization occurs at the boiling point.

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