energetics Flashcards

(12 cards)

1
Q

what is the definition of standard enthalpy change of formation?

A

enthalpy change when 1 mole of a substance is formed from its constituent elements with all reactants and products in standard states under standard conditions

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2
Q

what is the definition of standard enthalpy change of combustion?

A

enthalpy change when 1 mole of a substance is completely burnt in oxygen with all reactants and products in standard states under standard conditions

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3
Q

what is the definition of standard enthalpy change of neutralisation?

A

enthalpy change when 1 mole of water is formed in a reaction between an acid and alkali under standard conditions

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4
Q

what does each part of the q=mcΔT stand for?

A

q = energy required
m = mass of liquid heated
c = specific heat capacity of liquid
ΔT= temperature rise of liquid

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5
Q

what is the equation for calculating enthalpy change

A

ΔH=q divide moles in a reaction

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6
Q

1) In an experiment, 0.600 g of propane (C3H8) was completely burned in air. The heat evolved raised the temperature of 100 g of water by 64.9°C. Use this data to calculate the enthalpy of combustion of propane (the specific heat capacity of water is 4.18J g-1 K-1

A

1) q = mcΔT
m = 100
C=4.18
q = 100 x 4.18 x 64.9 = 27130 J (divide 1000 to get KJ)
ΔT = 64.9
ΔH = q / mol
moles of propane = mass / Mr
= 0.600 / 44.0 = 0.01364
ΔН = -27.13 / 0.01364 = -1990 kJ mol-1 (3 sig fig)

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7
Q

what is Hess’s law?

A

the enthalpy change for a reaction is independent of the route taken

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8
Q

why is the enthalpy change of formation of an element always 0?

A

don’t need energy to make an element

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9
Q

What is the Hess’s law on formation ?

A
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10
Q

What is the Hess’s law on combustion?

A
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11
Q

how do you calculate the ΔH using bond enthalpies?

A

ΔH= energy to break all bonds - energy to make all bonds
(reactants-products)

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12
Q

how to determine a more accurate value for the enthalpy of reaction

A
  1. insulate the beaker
  2. to reduce heat loss
  3. record temperature for a suitable time before adding the metal
  4. record the temperature values at regular intervals
  5. to plot the temperature results against the graph
  6. extrapolate the cooling back to the point of addition
  7. to establish a theoretical maximum temperature/ temp change
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