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CHEM 1A > Ch.6! > Flashcards

Ch.6! Flashcards

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1
Q

What is Energy?

A

Energy is the capacity to do work.

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2
Q

What is Work?

A

the result of a force acting through a distance.

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3
Q

What is heat?

A

the flow of energy caused by a temperature difference.

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4
Q

First Law of Thermochemistry:

A

Law of conservation of energy; energy cannot be created or destroyed.

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5
Q

what is a system? Examples?

A

the object of focus. coffee in a cup, piece of hot metal in water, etc.

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6
Q

what are surroundings? Examples?

A

Everything that a system can transfer its energy to. The cup holding the coffee, the water the hot metal is in, etc.

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7
Q

What is internal energy?

A

Sum of energies that compose the system.

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8
Q

What are the units associated with Energy?

A

Joules! 1 calorie=4.184J, 1 Calorie=4184J.

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9
Q

What is q(heat)? formula? rearranging formula?

A

q=mCΔT. C(specific heat capacity is dependent on chemical).

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10
Q

What is POSITIVE q?

A

absorbing energy (heat coming INTO the system.)

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11
Q

what is NEGATIVE q?

A

releasing energy (heat LEAVING the system)

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12
Q

What is a bomb calorimeter?

A

piece of equipment that measures Change in Energy for combustion reactions.

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13
Q

what is the formula for change in E of a calorimeter?

A

q(calorimeter)=C(calorimeter)xΔT or… q(calorimeter)=-q(rxn).

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14
Q

What is Enthalpy? (at constant pressure)

A

Enthalpy (of a system) as the sum of its internal energy and the product of its pressure and volume.

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15
Q

Enthalpy formula:

A

ΔH= q(p)

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16
Q

What is enthalpy a measure of?

A

ONLY heat exchanged under constant pressure!

17
Q

Endothermic reactions?

A

a chemical rxn with positive ΔH, ABSORBS heat from surroundings.

18
Q

EXOthermic reactions?

A

a chemical rxn with negative (-ΔH), GIVES heat to surroundings.

19
Q

Look over manipulating ΔHrxn, Hess’ Law!!!

A

yes.

20
Q

formula to calculate standard enthalpy of REACTION!

A

Δ H°rxn=(ΣΔ H°f(products)x(n))-(ΣΔ H°f(reactants)x(n)).

CHEM 1A (10 decks)

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