Magnesium undergoes reaction with dilute sulfuric acid. $\text{Mg}(s) + \text{H}_2\text{SO}_4(aq) \rightarrow \text{MgSO}_4(aq) + \text{H}_2(g)$ Two separate experiments are performed at $25^\circ\text{C}$. Experiment 1: $24.0\,\text{g}$ of powdered magnesium is reacted with $100\,\text{cm}^3$ of $1.0\,\text{mol dm}^{-3}$ sulfuric acid. Experiment 2: $24.0\,\text{g}$ of powdered magnesium is reacted with $50\,\text{cm}^3$ of $2.0\,\text{mol dm}^{-3}$ sulfuric acid. In each experiment, the volume of hydrogen formed is recorded. The outcomes are shown on a graph. Which graph is correct?
Chemistry 5070 · O Level · The mole and the Avogadro constant