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A student prepares an aqueous solution of ethanoic acid at The dissociation equilibrium is
At Figure 1 shows the initial concentration of ethanoic acid.
Using Figure 1, calculate the equilibrium concentration of Assume that Give your answer to three significant figures.
Use the equation in the data booklet to calculate in for the dissociation equilibrium at
State which side of the equilibrium is favoured.
In a sealed, fixed-volume vessel, nitrogen and oxygen form nitrogen monoxide at 1500 K:
N₂(g) + O₂(g) ⇌ 2NO(g)
At this temperature, Kc = 4.00 × 10⁻⁶. At a particular instant, the concentrations are [N₂] = 0.0500 mol dm⁻³, [O₂] = 0.0400 mol dm⁻³ and [NO] = 1.00 × 10⁻⁵ mol dm⁻³.
Calculate Qc for this mixture and predict the direction in which the reaction will proceed to reach equilibrium.
Determine the equilibrium concentrations of the three gases. Show how you check that any approximation used is justified.
After the mixture reaches equilibrium, an injection increases [NO] by 2.00 × 10⁻⁴ mol dm⁻³. Immediately after the injection, before further reaction occurs, calculate Qc and predict the direction in which the reaction will proceed.
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