Reactivity 1.4 (HL) Flashcards

1
Q

Entropy (S)

A

Measure of the ways in which the available energy of a system can be distributed among the particles of a system (JK-1 mol-1)

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2
Q

Can entropy be measured?

A

Yes, absolute values can be measured

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3
Q

Why would entropy increase (4 ways)

A
  • Mixing different states
  • Increasing distance between particles (changing state)
  • Increasing movement of particles (increasing temperature)
  • Increasing the number of particles (mol ratio)
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4
Q

Entropy change formula

A

Differences between the total entropy of the products and the total entropy of the reactants (Sp - Sr)

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5
Q

Gibbs Energy Change (g)

A

Energy obtained from a chemical reaction that is available to do work (kj mol-1)

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6
Q

Value of G

A

Always negative as it is energy obtained

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7
Q

Gibbs energy change formula

A

G = H - T S

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8
Q

Spontaneous reaction

A

System becomes more stable (able to do work) Once started, it does not need any additional energy. G must be negative

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9
Q

Reaction Quotient (Q)

A

Ratio of products and reactants concentration when not at equilibrium

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10
Q

Equilibrium constant (K)

A

Value of the reaction quotient in equlibrium.

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11
Q

When is K=0?

A

G is greater than 30kj mol-1
No reaction - impossible.

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12
Q

When is K smaller than 1?

A

G is between 0 and 30 kjmol1
Partial reaction occurs

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13
Q

When is K=1?

A

When G=0
Partial reaction occurs

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14
Q

When is K greater than 1?

A

G is greater than 0 and 30kjmol
Partial reaction occurs

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15
Q

When is K»1?

A

G is smaller than -30kjmol
Complete reaction occurs

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