DF1 - Thermochemistry Flashcards

Getting energy from fuels

1
Q

Define ‘thermochemistry’.

A

The study of energy and heat associated with chemical reactions

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2
Q

Define ‘exothermic’.

A

A reaction that gives out energy and heats surroundings

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3
Q

During an exothermic reaction, are bonds formed or broken?

A

Formed

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4
Q

During an exothermic reaction, is energy released or taken in?

A

Released

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5
Q

Where does energy released from an exothermic reaction go?

A

It’s lost to the reaction’s surroundings and heats them up

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6
Q

Is enthalpy change positive/negative for exothermic reactions and why?

A

Negative - products end up with less energy than reactants

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7
Q

Define ‘endothermic’.

A

A reaction that takes in energy and cools the surroundings

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8
Q

During an endothermic reaction, are bonds formed or broken?

A

Broken

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9
Q

Is enthalpy change positive/negative for endothermic reactions and why?

A

Positive - products end up with more energy than reactants

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10
Q

Define ‘enthalpy change’.

A

Amount of energy transferred to and from surroundings

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11
Q

Why are standard conditions used when calculating enthalpy change?

A

They are set conditions which allows us to compare enthalpy changes

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12
Q

What temperature is used in standard conditions?

A

298K

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13
Q

What pressure is used in standard conditions?

A

1atm

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14
Q

What concentration is used in standard conditions?

A

1 moldm-3

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15
Q

How do you convert K to degrees C?

A

Minus 273

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16
Q

What are the 4 types of enthalpy change?

A
  • Standard enthalpy change of a reaction
  • Standard enthalpy change of formation
  • Standard enthalpy change of combustion
  • Standard enthalpy change of neutralisation