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For the equation:- $ch_{3}ch_{3}oh_{(aq)}+ch_{3}cooh_{(aq)}rightleftharpoons CH_{3}COOOH_{3}CH_{3}(aq)+H_{2}O(l)$ Calculate the mass of ethanoic acid that must be mixed with 20 moles of ethanol to produce 1.5 moles of ethyl ethanoate at equilibrium. (8 marks)
Accepted Answer
The provided equation represents the esterification reaction between ethanol and ethanoic acid to produce ethyl ethanoate and water. Here's how to solve the problem:
1. Write the equilibrium constant expression:
K = [CH3COOCH3] [H2O] / [CH3CH2OH] [CH3COOH]
2. Set up an ICE table:
| | CH3CH2OH | CH3COOH | CH3COOCH3 | H2O |
|----------- |----------|---------|------------|------|
| Initial | 20 | x | 0 | 0 |
| Change | -1.5 | -1.5 | +1.5 | +1.5 |
| Equilibrium | 18.5 | x - 1.5 | 1.5 | 1.5 |
3. Substitute the equilibrium concentrations into the K expression:
K = (1.5)(1.5) / (18.5)(x - 1.5)
4. Solve for x (the initial concentration of ethanoic acid):
You will need the value of the equilibrium constant (K) for the reaction. It is not provided in the problem. You would need to look it up or be given it.
Once you have K, solve the equation for x.
5. Calculate the mass of ethanoic acid:
mass = moles x molar mass
mass = x (moles of ethanoic acid) x 60.05 g/mol (molar mass of ethanoic acid)
Note: The exact answer depends on the value of the equilibrium constant (K).
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