Practice Scenario 2: Calculating Equilibrium Concentrations/partial Pressures From Initial Conditions And K (ice Tables) (6.3.2)

Practice: Scenario 2: Calculating Equilibrium Concentrations/Partial Pressures from Initial Conditions and K (ICE Tables)

Lesson 6.3.2Equilibrium

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9 questions

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6 sample questions

Question 1.
If 2.0 mol of A is placed in a 5.0 dm³ container, what is the initial concentration of A?
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Use the formula: concentration = moles/volume.
Question 2.
In the reaction C ⇌ D, if the initial concentration of D is 0.20 mol/dm³ and no C is present, write the initial conditions in an ICE table.
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Remember to fill out all initial values for the ICE table.
3Question 3.
What does the 'I' in ICE stand for?
- Changes
- Initial
- Equilibrium
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Think about what you record first on the table.
4Question 4.
Is the reaction PCl₅ ⇌ PCl₃ + Cl₂ reversible?
- True
- False
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Consider the nature of decomposition reactions.
Question 5.
If you start with 0.40 mol of C in a 2.0 dm³ container, and the reaction C ⇌ 2D has Kc = 0.1, calculate equilibrium concentrations using ICE.
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Make sure your expressions for changes reflect the stoichiometry.
Question 6.
For the reaction N₂ + 3H₂ ⇌ 2NH₃, starting with 1.0 mol of N₂ in a 5.0 dm³ and with Kc = 0.3, calculate equilibrium concentrations.
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Consider if an approximation is valid before performing calculations.

5 more questions in this section. Enroll free to practise them all.