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Chemical equilibria, Le Chatelier’s principle and $K_c$

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Question 4

Species D\text{D}D and E\text{E}E react together in aqueous solution to form an equilibrium mixture according to the following equation:

D(aq)+2E(aq)⇌F(aq) \text{D}(aq) + 2\text{E}(aq) \rightleftharpoons \text{F}(aq) D(aq)+2E(aq)⇌F(aq)
a.

An aqueous solution containing 0.60 mol of D\text{D}D is mixed with an aqueous solution containing 0.50 mol of E\text{E}E.

When equilibrium is reached, the mixture contains 0.060 mol of F\text{F}F.

Calculate the amount of D\text{D}D and the amount of E\text{E}E, in moles, in this equilibrium mixture.

[3]
b.

At a different temperature, another equilibrium mixture of these species in a 500 cm3 flask contains 0.30 mol of D\text{D}D, 0.45 mol of E\text{E}E, and 0.080 mol of F\text{F}F.

Calculate the value of the equilibrium constant Kc K_c\,Kc​ at this temperature and deduce its units.

[5]

Chemical equilibria, Le Chatelier’s principle and $K_c$ Questions

  1. A Level
  2. /Chemistry
  3. /Chemical equilibria, Le Chatelier’s principle and $K_c$