module 3: 9.1 enthalpy changes Flashcards

3.2.1 enthalpy changes

1
Q

define the term enthalpy

A

enthalpy (H) is a measure of the heat content or energy in a chemical system. The chemical system refers to the atoms, molecules or ions making up the chemicals.

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2
Q

what is an exothermic change

A
  • from the system to the surroundings, it releases heat energy to the surroundings.
  • Delta H is negative
  • The temperature of the surroundings increase as they gain energy (temp increase)
  • Reactants is higher than products
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3
Q

what is an endothermic change

A
  • from the surroundings to the system, it takes in heat energy from the surroundings
  • Delta H is positive
  • The temperature of the surroundings decrease as they lost energy (temp decrease)
  • Reactants is lower than products
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4
Q

define the term activation energy

A

the energy required to break bonds acts as an energy to the reaction, known as activation energy E (subscript) a
It is the minimum energy needed for the reaction to take place

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5
Q

what are the standard conditions

A
  • standard pressure - 100 kPa
  • standard temperature - 25 degrees C or 298 K
  • standard concentration - 1 mol dm-3
    standard state - physical state under standard conditions
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6
Q

define the standard enthalpy change of reaction

A

the standard enthalpy change of reaction (ΔrH^⦵) is the enthalpy change that accompanies a reaction in the molar quantities shown in a chemical equation under standard conditions, with all reactants and produces in their standard states

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7
Q

define the enthalpy change of formation

A

the standard enthalpy change of formation (ΔfH^⦵) is the enthalpy change that takes place when one mole of a compound is formed from its elements under standard conditions, with all reactants and products in their standard states

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8
Q

define enthalpy change of combustion

A

the standard enthalpy change of combustion (ΔcH^⦵) is the enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, with all reactants and products in their standard states.

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9
Q

define enthalpy change of neutralisation

A

the standard enthalpy change of neutralisation (ΔneutH^⦵) is the energy change that accompanies the reaction of an acid by a base to form one mole of H20 (l), under standard conditions, with all reactants and products in their standard states.

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10
Q

formula for energy (Q)

A
Q = mcΔT
q - energy (J)
m - mass of water
c  - 4.18 (J/g/ degrees C or K)
ΔT - Change in temperature (degrees C)
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