Equilibria flashcards

1
Q

How does a closed system differ from an open system?

A

A closed system does not exchange matter with its surroundings, while an open system does.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is dynamic equilibrium?

A

A state where the forward and reverse reaction rates are equal, and concentrations remain constant.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How does increasing temperature affect an exothermic reaction at equilibrium?

A

It shifts equilibrium to favour the reactants (left).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How does increasing pressure affect a gaseous equilibrium?

A

The system shifts to the side with fewer gas molecules.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the equilibrium constant (K)?

A

A ratio that expresses the relative concentrations of products to reactants at equilibrium.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What happens if a catalyst is added to an equilibrium system?

A

It speeds up both forward and reverse reactions but does not change equilibrium position.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How does activation energy influence reversibility?

A

Lower activation energy makes reversibility more likely; high activation energy favours irreversibility.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What must happen for dynamic equilibrium to be reached?

A

The forward and reverse reaction rates must be equal, and concentrations must remain constant.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How does the rate of the forward reaction change over time?

A

It decreases as reactants are consumed.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How does the rate of the reverse reaction change over time?
A: It increases as products are formed.

A

It increases as products are formed.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How does temperature affect K?

A

For exothermic reactions, K decreases with temperature increase; for endothermic reactions, K increases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the reaction quotient (Q)?

A

A ratio of product/reactant concentrations at any point, not necessarily equilibrium.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What does it mean if:
-Q = K
-Q > K
-Q < K

A

Q = K system is at equilibrium
Q > K reaction shifts left (reverse reaction favoured)
Q < K reaction shifts right (forward reaction favoured)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

If K is large, what does that indicate?

A

The reaction heavily favours products.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

If K is small, what does that indicate?

A

The reaction heavily favours reactants.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How does adding a reactant affect equilibrium?

A

It shifts right (forward reaction favored).

17
Q

How does removing a reactant affect equilibrium?

A

It shifts left (reverse reaction favored).