CHEM105 PASS Week 10

PASS CHEM105

Question Time

ft. Tim Tams + stock images

Warm up Qs

Written Qs

Your Qs

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Today's PASS session

Multiple Choice

The concentration value of 5.0M can also be expressed as:

• 5.0mol

• 5.0mol/g

• 5.ml/mol

• 5mol/L

Multiple Choice

Consider the equilibrium: 2NO2(g) ↔ N2O4(g) ∆H = -58.2 kJ

At room temperature NO2 is brown and N2O4 is colourless.

When the sealed flask containing gases is submerged in cold water

• The brown colour increases

• The brown colour decreases

• The intensity of the brown colour remains the same

• . The intensity of the colour cannot be predicted

Multiple Choice

Ag+ ions react with Fe2+ ions according to the equation:

Ag+ (aq) + Fe2+ (aq) ↔ Ag(s) + Fe3+ (aq)

The concentration of Ag+ at equilibrium is not changed by adding:

• Fe2+ (aq)

• Ag(s)

• Ag+ (aq)

• Cl- (aq)

​​Are we feeling warm?

Consider the image to the right.

Using the information that you have, provide a written response to

justify whether this is a reactant, or

product favoured reaction.

In your answer you must make reference to the equilibrium constant (3 marks)

Consider the graph to the right.

Provide a written response about the

substances represented by each line

that describes what is happening to

their concentration.

Your answer must include discussion of

chemical equilibrium (4 marks).

Consider the equation below (not the dog).

What would happen to the equilibrium if this reaction took place in a smaller container? Provide a written response that includes which way the equilibrium would shift, and reference the appropriate Gas law (3 marks)

Sorry, you're not done.

Now, what would happen to the equilibrium of this equation if pressure were to increase?

Dog says you smashed it!