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1. How would using double the volume of hydrochloric acid have affected the empirical formula of zinc chloride? 2. Suppose that you had not driven off all the water from the zinc chloride. How would t...

1. How would using double the volume of hydrochloric acid have affected the empirical formula of zinc chloride?

2. Suppose that you had not driven off all the water from the zinc chloride. How would this error have affected the empirical formula for zinc chloride?

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Answer #1

Your tool of choice here will be the mole ratio that exists between zinc metal, Zn, and hydrochloric acid, :HCl, in the balanced chemical equation.

Zn(s]+2HCl(aq]→ZnCl2(aq]+H2(g]↑⏐

You're dealing with a single replacement reaction in which zinc displaces the hydrogen from hydrochloric acid. The products of the reaction are aqueous zinc chloride and hydrogen gas.

Now, as you can see from the balance chemical equation, a 1:2 mole ratio exists between the two reactants.

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