energetics Flashcards

1
Q

define an exothermic reaction

A

energy has been given out of the reaction

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2
Q

define endothermic reaction

A

energy has been taken into the reaction

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3
Q

give one example of an exothermic reaction

A

neutralising an acid with an alkali

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4
Q

give an example of an endothermic reaction

A

making white anhydrous copper sulfate and water from blue copper sulfate

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5
Q

define enthalpy change

A

measuring a heat change at a constant pressure

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6
Q

what are the standard conditions for measuring enthalpy changes

A

100 kPa
298 K

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7
Q

why are exothermic reactions given a negative sign (-)

A

the products end up with less heat energy than the reactant as they lost energy when they heated up their surroundings. this means enthalpy change is negative

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8
Q

what are energy level diagrams used to show

A

enthalpy change

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9
Q

what is enthalpy change measured in

A

kJ per mole (mol-1)

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10
Q

define enthalpy of formation

A

the enthalpy change when one mole of substance is formed from its consistuent elements under standard condition, all reactants and products being in their standard states

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11
Q

define enthalpy of combustion

A

the enthalpy change when one mole of substance is completely burnt in oxygen under standard conditions, all reactants and products being in their standard states

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12
Q

define specific heat capacity

A

the amount of heat needed to raise the temperature of 1g of substance by 1K

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13
Q

what is the equation for calorimetry

A

Q = mc delta t

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14
Q

what is calorimetry used for

A

to compare the values of enthalpy change for a series of similar compounds because the errors will be similar for every experiment

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15
Q

how is a flame calorimeter better than a simple calorimeter

A

the spiral chimney is made of copper

the flame is enclosed

fuel burns in pure oxygen

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16
Q

what is a displacement reaction

A

a metal that is more reactive than another will displace the less reactive one from a compound

17
Q

how do you minimise the effects of heat lost from a polystyrene cup

A

plotting a cooling curve

18
Q

define Hess’ law

A

the enthalpy change for a reaction is the same independent of the route taken from reactants to products

19
Q

define enthalpy change

A

A heat change at constant pressure

20
Q

what is the difference between heat and temperature

A

temperature - related to the average kinetic energy of the particles in a system but is independent to the number of particles present

heat- a measure of the total energy of all of the particles present in a given amount of substance and is dependent on the number of particles

21
Q

what are the 3 things you need in order to measure the enthalpy change of a reaction

A
  1. mass of the substance that is being heated up or cooled down
  2. temperature change
  3. specific heat capacity of the substance
22
Q

what is the equation for enthalpy change

A

q = mc Δ T

23
Q

why are neutralisation reactions exothermic

A

they give out heat

24
Q

state the method that allows for heat loss in the enthalpy change practical

A
  • Place 50 cm cubed of 1.0 mol dm-3 hydrochloric acid in a polystyrene cup and 50 cm cubed of 1.0 mol dm-3 sodium hydroxide in another
    2. using a thermometer with 0.1 degrees increments take the temperature of each solution every 30 seconds for 4 minutes to confirm that both solutions remain at the same temperature as the laboratory
    3. Plot a cooling graph and draw a line of best fit through these points
    3. now pour the solution into the other and stir continuously and record the temperature every 30 seconds for 6 minutes
25
Q
A