Chemical Energetics Flashcards

1
Q

Hess’ Law

A

The enthalpy change accompanying a chemical reaction is the same REGARDLESS OF THE ROUTE by which the chemical change occurs, provided the INITIAL AND FINAL STATES ARE THE SAME.

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2
Q

STANDARD enthalpy change of reaction

A

The energy change in a chemical reaction when MOLAR QUANTITIES OF REACTANTS specified in the chemical equation react to form products at STANDARD CONDITIONS

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3
Q

Standard enthalpy change of formation of substance (this feels like the more general one to me because it could be any substance)

A

The energy change when ONE MOLE OF THE SUBSTANCE is formed from its CONSTITUENT ELEMENTS under standard conditions.

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4
Q

Standard enthalpy change of combustion a substance

A

Is the energy evolved when one mole of a substance is COMPLETELY BURNT IN OXYGEN under standard conditions.

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5
Q

Standard enthalpy change of neutralisation

A

Is the energy evolved when ONE MOLE OF WATER is formed from the neutralisation between an acid and a base under standard conditions. (omg neutralisation is exothermic)

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6
Q

Standard enthalpy change of atomisation of an element

A

Is the energy ABSORBED when one mole of gaseous ATOMS is formed from the element under standard conditions.

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7
Q

Bond energy

A

The AVERAGE energy that is absorbed to break one mole of covalent bonds in the GASEOUS STATE to form GASEOUS ATOMS under standard conditions.

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8
Q

Bond dissociation energy

A

The energy required to break ONE MOLE OF A PARTICULAR COVALENT BOND in a SPECIFIC MOLECULE in the gaseous state to form gaseous atoms.

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9
Q

Lattice energy of an ionic solid

A

Energy evolved when one mole of a SOLID IONIC COMPOUND is formed from its constituent GASEOUS IONS under standard conditions.

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10
Q

First ionisation energy

A

The energy absorbed when one mole of GASEOUS atoms loses one mole of electrons to form one mole of singly charged GASEOUS cations.

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11
Q

Second ionisation energy

A

The energy absorbed when one mole of singly charged gaseous cations loses one mole of electrons to form one mole of doubly charged gaseous cations.

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12
Q

First electron affinity

A

The energy released when one mole of gaseous atoms acquires one mole of electrons to form one mole of singly charged gaseous anions.

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13
Q

Second electron affinity

A

The energy absorbed when one mole of singly charged gaseous anions acquires one mole of electrons to form one mole of doubly charged gaseous anions.

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14
Q

Standard enthalpy change of hydration of an ion

A

Energy EVOLVED when one mole of gaseous ions is HYDRATED under standard conditions.

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15
Q

Standard enthalpy change of solution of a substance

A

Energy change when one mole of a substance is completely dissolved in a solvent to form an INFINITELY DILUTE SOLUTION under standard conditions.

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16
Q

Define entropy

A

Measures the DEGREE OF DISORDER or randomness in a system. It is reflected in the number of ways the ENERGY in a system can be DISTRIBUTED through the MOTION OF THE PARTICLES.

17
Q

When does entropy change?

A
  • When there is a change in phase*
  • When there is a change in temperature
  • When there is a change in the number of particles*
  • When a gaseous system faces an expansion of volume
  • When particles are mixed
    Depends on the number of ways to distribute the particles and energy