P1: Energetics Flashcards

Bond energy, Hess's Law

1
Q

What is enthalpy?

A

Refers to all the heat energy stored in a chemical system,under constant pressure

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2
Q

What is enthalpy change? (🔺H)

A

When you measure a heat energy change under a constant pressure

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3
Q

What is Hess’s Law?

A

The enthalpy change in a reaction at constant pressure is independent of the route taken.

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4
Q

What are the standard conditions?

A

100KPa
298K (25•c)

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5
Q

Describe a formation cycle

A

🔺cH/🔺rH
Reactants ——> Products
^. ^. 🔺fH
^. ^
Elements in their
Standard states

  1. Balance equation for direct route
  2. Draw thermochemical cycle and note which arrow you flip
  3. Calculate total enthalpy change of formations for reactants and products (ignoring H) (times moles)
  4. Add formation values to cycle and flip the sign of the arrow you flipped.
  5. Sum them together

(this is for each element)

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6
Q

Describe a Combustion Cycle

A

🔺fH/🔺rH
Reactants ————> Products
v. v 🔺cH
v. v
Combustion products
CO2+ H2O

  1. Draw combustion cycle and balance equations
  2. Using the date from the table, replace 🔺cH with the combustion values (times any moles)
    (O2 is not included)
  3. Flip the symbol (+ or -) if the route
    goes against the arrow
  4. Add 🔺cH together to find 🔺fH
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7
Q

What equation do you use to find energy?

A

q= mc🔺t

q= energy ( j )
m= mass (g)
c= SHC (4.18Jg^-1K^-1)
t= temp change (K)

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8
Q

How do you find an enthalpy value?

A

Enthalpy = energy/moles

  1. Find energy
    q=mc🔺t
  2. Find moles
    moles= mass/Mr
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9
Q

What is Calorimetry used for?

A

To work out the enthalpy change of combustion

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10
Q

Describe the procedure to find the enthalpy change in a solution

A

-Use a polystyrene cup to prevent heat loss
-Add the acid and measure the temperature
-Add the alkali, stir, measure the temperature change
-Use q=mc🔺t (add mass of acid and alkali)
-Use mol= conc x vol
- Enthalpy= q/mol

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11
Q

Define standard enthalpy change of reaction (🔺rH)

A

The enthalpy change of reaction according to the molar quantities in the equation under standard conditions

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12
Q

Define standard enthalpy change of formation (🔺fH)

A

Enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions

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13
Q

Define standard enthalpy change of combustion (🔺cH)

A

Enthalpy change when 1 mole of a substance is completely burnt in oxygen to make CO2 and H2O, under standard conditions

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14
Q

Define standard enthalpy change of neutralisation (🔺neaut H)

A

Enthalpy change when an acid and an alkali react to form 1 mole of water under standard conditions

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15
Q

What is an exothermic reaction?

A

-Give out heat energy to surroundings
-Gets hotter
-Make bonds
-Negative value

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16
Q

What is an endothermic reaction?

A

-Absorbs heat energy from surroundings
-Gets colder
-Breaks bonds
-Positive bonds

17
Q

Describe an exothermic energy level diagram

A

-Reactant line at top
-Arrow down
-Products line at bottom

18
Q

Describe an endothermic energy level diagram

A

-Reactant line at bottom
-Arrow up
-Products line at top

19
Q

🔺H is…
and is measured in…

A

Enthalpy change
Measured in joules (J)

20
Q

What is on the x and y axis of an energy level diagram?

A

x= progress of reaction
y= energy

21
Q

What is different about an enthalpy level diagram compared to and energy level diagram?

A

Same but:
-Arrow is labelled with 🔺H=
-y axis is enthalpy

22
Q
A