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Enthalpy Changes Flashcards

(12 cards)

1
Q

Use ideas about the enthalpy changes that take place during bond breaking and bond making to explain why some reactions are exothermic

A

Bond breaking absorbs energy and bond making releases energy. More energy is released than absorbed.

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2
Q

If the products of a reaction is carbon dioxide and water, what name is given to this oxidation process in the body?

A

Respiration

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3
Q

If the products in a reaction is glucose and oxygen, what is the name of the oxidation process in the body?

A

Photosynthesis

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4
Q

What is the equation to work out energy released?

A

q = m x c x T(change in temperature)

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5
Q

Suggest two reasons why standard enthalpy changes of combustion determined experimentally are less exothermic than the calculated theoretical values

A
  • Heat is released to surroundings

- Non-standard conditions

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6
Q

State Le Chatelier’s principle

A

The position of equilibrium will shift, minimising the effect of any change in conditions and counteracting the change

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7
Q

Define the term enthalpy change of combustion

A

The enthalpy change when one mole of substance is burnt in excess oxygen under standard conditions (100kPa and 25 degrees C)

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8
Q

What are the standard condition?

A

100kPa and 25 degrees C

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9
Q

It is very difficult to determine the standard enthalpy change of formation of hexane directly. Suggest a reason why.

A
  • Many hydrocarbons would form

- Activation energy is too high

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10
Q

Why do bond enthalpies have positive values?

A

Bond breaking is endothermic so energy has to be put in to break the bond

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11
Q

Define the term enthalpy change of formation

A

The enthalpy change when one mole of compound is formed from its elements under standard conditions (100kPa and 25 degrees C)

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12
Q

What are the conditions indicated by the circle with the line through it?

A

Standard conditions meaning 100kPa and 25 degrees C

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