In the following reaction: #Mg(s) + 2H_2O(l) -> Mg(OH)_2(s) + H_2(g)#. What mass of Mg must you use to make #5.6 x 10^4#g of #Mg(OH)_2#?
The given equation correctly identifies the molar equivalence of reactants and products. One mole of metal reduces two moles of water, and yields PRECISELY 1 mole of metal hydroxide. In practice, you would need a fair bit of heat (and activated metal) to make this go. We
And thus moles of
And so we need the following mass of metal:
Magnesium hydroxide is part of our pharmacopeia, and is administered as