How Far? The Extent of Chemical Change · Paper 1 — Free Chemistry SL Practice Questions

For the esterification reaction $$\text{CH}_3\text{COOH}(\text{l}) + \text{C}_2\text{H}_5\text{OH}(\text{l}) \rightleftharpoons \text{CH}_3\text{COOC}_2\text{H}_5(\text{l}) + \text{H}_2\text{O}(\text{l}),$$ a student mixes $2.0\ \text{mol}$ of ethanoic acid with $2.0\ \text{mol}$ of ethanol in a $1.0\ \text{dm}^3$ flask. At equilibrium, $1.2\ \text{mol}$ of ethyl ethanoate is present. What is the value of $K_c$?

For the equilibrium $\text{N}_2\text{(g)} + 3\text{H}_2\text{(g)} \rightleftharpoons 2\text{NH}_3\text{(g)}$, the equilibrium concentrations are $[\text{N}_2] = 0.50 \ \text{mol dm}^{-3}$, $[\text{H}_2] = 0.20 \ \text{mol dm}^{-3}$, and $[\text{NH}_3] = 0.40 \ \text{mol dm}^{-3}$. What is the value of $K_c$?

In an experiment, $0.800\ \text{mol}$ of $\text{HI}(g)$ is placed in a $1.00\ \text{dm}^3$ container and allowed to reach equilibrium according to the equation: $$2\text{HI}(g) \rightleftharpoons \text{H}_2(g) + \text{I}_2(g)$$ At equilibrium, $[\text{I}_2] = 0.150\ \text{mol dm}^{-3}$. What is the value of $K_c$?

For the equilibrium $\text{N}_2\text{(g)} + 3\text{H}_2\text{(g)} \rightleftharpoons 2\text{NH}_3\text{(g)}$, a $1.00\ \text{dm}^3$ vessel initially contains $0.500\ \text{mol}$ of $\text{N}_2$ and $1.500\ \text{mol}$ of $\text{H}_2$. At equilibrium, $[\text{NH}_3] = 0.200\ \text{mol dm}^{-3}$. What is the value of $K_c$?