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LeChatelier

Total questions: 12

Worksheet time: 10mins

Name

Class

Date

For the reaction N₂(g) + 3H₂(g) <--> 2NH₃(g) + 92 kJ;

what happens to the concentration of N2 when heating up the chamber this takes place in?

concentration of nitrogen increases

concentration of nitrogen decreases

concentration of nitrogen stays the same

For the reaction N₂(g) + 3H₂(g) <--> 2NH₃(g) + 92 kJ;

what happens to the equilibrium position by adding a catalyst to this reaction?

Shifts to the left (reactants)

Shifts to the right (products)

No effect

Which system at equilibrium will be least affected by a change in pressure?

3 H2(g) + N2(g) ↔ 2 NH3(g)

2 S(s) + 3 O2(g) ↔ 2 SO3(g)

AgCl(s) ↔ Ag+(aq) + Cl– (aq)

2 HgO(s) ↔ 2 Hg(g) + O2(g)

Given the reaction: $N_{2\left(g\right)}+O_{2\left(g\right)}+182.6kJ\ \ ↔\ \ 2NO_{\left(g\right)}$
Which change would cause an immediate increase in the rate of the forward reaction (i.e., cause shift toward products)?

increasing the concentration of NO(g)

increasing the concentration of N2(g)

decreasing the reaction temperature

decreasing the reaction pressure

Which of the two graphs reaches equilibrium?

The left one.

The right one.

Both of them.

Neither.

For the reaction...

H_{2 (g)} + Cl_{2 (g)}<=> 2HCl _(g) + heat

If the pressure in the system is increased, the equilibrium position will _______.

shift to the left

shift to the right

not shift position at