The equation for the reaction between aluminium and hydrochloric acid is
2Al(s)+6HCl(aq)→2AlCl3(aq)+3H2(g) 2\text{Al(s)} + 6\text{HCl(aq)} \rightarrow 2\text{AlCl}_3\text{(aq)} + 3\text{H}_2\text{(g)} 2Al(s)+6HCl(aq)→2AlCl3(aq)+3H2(g)What is the minimum mass, in mg, of aluminium (Ar=27.0A_{\text{r}} = 27.0Ar=27.0) needed to react completely with 45.0 cm3 of 0.800 mol dm-3 hydrochloric acid?
3.24×10−13.24 \times 10^{-1}3.24×10−1
3.24×1023.24 \times 10^23.24×102
9.72×1029.72 \times 10^29.72×102
2.92×1032.92 \times 10^32.92×103