Chemical Energy Flashcards

1
Q

What is the change in energy in a chemical reaction known as ?

A

the enthalpy change

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2
Q

What does a highly exothermic reaction require ?

A

cooling as a lot of heat energy will be released

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3
Q

What does a highly endothermic reaction require?

A

infrastructure to supply heat to maintain the reaction

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4
Q

What is the experimental set up for calculating the energy released by a fuel such as an alcohol?

A
tripod
burning fuel
water 
copper cup
thermometer
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5
Q

What calculation can be used to calculate the energy transferred to the water when measuring the energy released by a fuel?

A
E= cm^t
^ = delta
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6
Q

What must the mass of water be in?

A

KILOGRAMS (1kg = 1000g)

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7
Q

What is the enthalpy of the combustion of substance?

A

the heat energy released when 1 mole of a substance burns completely in oxygen

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8
Q

What must you remember about the enthalpy change for an exothermic reaction?

A

it is negative and heat energy is released to surroundings

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9
Q

What is the equation used to find the temperature increase?

A

^T=Eh/cm

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10
Q

Why might the theoretical enthalpy of combustion be greater than the experimental value?(3)

A

heat loss to surroundings
incomplete combustion of (ethanol)
loss of (ethanol) through evaporation

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11
Q

What does Hess’ law state?

A

the enthalpy of a reaction is independent on the chemical route taken

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12
Q

What is the equation according to Hess’law following the formation of carbon dioxide?

A

^H= ^H1+^H2

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13
Q

To understand Hess’ law, what enthalpy equations must be considered?

A

enthalpy of combustion

enthalpy of formation

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14
Q

What must you remember about enthalpy of formation?

A

only 1 mole of a substance is being produced from its elements

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15
Q

What can bond enthalpies be used to estimate?

A

the enthalpy change occuring for a gas phase reaction by calculating the energy required to break bonds in reactants and the energy released when new bonds are formed in the products

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16
Q

What does the term ‘mean bond entahply’ refer to?

A

the average energy values to break one mole of bonds which occur in different molecules