Chapter 9 Flashcards

1
Q

What is the definition of enthalpy?

A

Is the measure of heat energy present in a chemical system (H)

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2
Q

What is the definition of enthalpy change?

A

Is the amount of energy released/taken in during a reaction (ΔH)

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3
Q

Are the energy changes +ive or -ive for exo and endothermic reactions?

A

-ive change is exothermic, +ive change is endothermic

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4
Q

What are standard conditions for enthalpy changes?

A

100KPa, 298K (25°C), 1moldm^-3, and standard state (the physical state of a substance under standard conditions)

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5
Q

Definition of standard enthalpy change of a reaction.

A

The energy change associated with a chemical reaction in the molar quantities under standard conditions.

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6
Q

Definition of standard enthalpy change of formation.

A

The energy change associated with the formation of 1 mole of a compound from its elements, under standard conditions. (The ΔfH of an element is 0)

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7
Q

Definition of standard enthalpy change of combustion.

A

The energy change associated with the complete combustion of 1 mole of a substance, under standard conditions

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8
Q

Definition of standard enthalpy change of neutralisation.

A

The energy change associated with the formation of 1 mole of water from a neutralisation reaction between and acid and base, under standard conditions. (Always ΔneutH for acid+base = -57mol^-1)

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9
Q

What are possible accuracy issues for ΔcH?

A

Heat loss to the surroundings, incomplete combustion, evaporation of fuel, not under standard conditions

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10
Q

Definition of average bond enthalpy.

A

The energy required to break one mole of a specified type of bond in a gaseous molecule (higher the value, stronger the bond)

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11
Q

Why would a reaction be exothermic?

A

Making the bonds releases more energy than was required for breaking the bonds.

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12
Q

What does Hess’ Law state?

A

If a reaction can take place by two routes, and the starting and finishing conditions are the same, the total energy enthalpy change is the same

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