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skelet666 [1.2K]
3 years ago
12

Consider four different samples: aqueous LiBr , molten LiBr , aqueous AgBr , and molten AgBr . Current run through each sample p

roduces one of the following products at the cathode: solid lithium, solid silver, or hydrogen gas. Match each sample to its cathodic product.Math following to Cathoid Products-Solid Lithium, Solid Silver, and Hydrogen GasSamples1. Aqueous LiBr2. Molten LiBr3. Aqueous AgBr4. Molten AgBr
Chemistry
1 answer:
Charra [1.4K]3 years ago
6 0

Answer:

a) Aqueous LiBr = Hydrogen Gas

b) Aqueous AgBr = solid Ag

c) Molten LiBr = solid Li

c) Molten AgBr = Solid Ag

Explanation:

a) Aqueous LiBr

This sample produces Hydrogen gas, because the H+ (conteined in the water) has a reduction potential higher than the Li+ from the salt. Therefore the hydrogen cation will reduce instead of the lithium one and form the gas.

b) Aqueous AgBr

This sample produces Solid Ag, because the Ag+ has a reduction potential higher than the H+ from the water. Therefore the silver cation will reduce instead of the hydrogen one and form the solid.

c) Molten LiBr

In a molten binary salt like LiBr there is only one cation present in the cathod. In this case the Li+, so it will reduce and form solid Li.  

c) Molten AgBr

The same as the item above: there is only one cation present in the cathod. In this case the Ag+, so it will reduce and form solid Ag.  

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Balanced chemical reaction

                 4Fe  +  3O₂  ⇒   2Fe₂O₃

a.- Calculate the moles of Fe₂O₃

                 4 moles of Fe ----------------- 2 moles of Fe₂O₃

                16.7 moles of Fe --------------  x

                                    x = (16.7 x 2)/4

                                    x = 33.4/4

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c.- Convert moles to mass

                       160 g of Fe₂O₃ ------------ 1 mol

                          x                     ------------ 8.35 moles of Fe₂O₃

                          x = (8.35 x 160)/1

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moles of H₃PO₄ = ?

mass of P₄O₁₀ = 71 g

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