Can someone explain and answer this question???
Zn(s) + HgCl2(aq) ZnCl2(aq) + Hg(l)
Zinc reacts with mercury(II) chloride to produce zinc chloride and mercury as shown above. Assume the reaction goes to completion and the density of Hg(l) is 13.55 g/mL. What volume of liquid mercury can be produced if 0.3970 moles of zinc are reacted with 0.2890 moles of mercury(II) chloride?
Zn(s) + HgCl2(aq) ZnCl2(aq) + Hg(l)
Zinc reacts with mercury(II) chloride to produce zinc chloride and mercury as shown above. Assume the reaction goes to completion and the density of Hg(l) is 13.55 g/mL. What volume of liquid mercury can be produced if 0.3970 moles of zinc are reacted with 0.2890 moles of mercury(II) chloride?
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The mole ratio is one to one between Zn and HgCl2
therefore HgCl2 is the limiting reactant:
0.2890mol HgCl2(1mol Hg/1mol HgCl2)(200.59g/mol)
(1ml/13.55g) = 4.278ml with 4 sig figs.
therefore HgCl2 is the limiting reactant:
0.2890mol HgCl2(1mol Hg/1mol HgCl2)(200.59g/mol)
(1ml/13.55g) = 4.278ml with 4 sig figs.