Problem

From the balanced molecular equations, write the …

02:33

Problem 10 Medium Difficulty

A novel process for obtaining magnnesium from sea water involves s. Write a balanced chemical
equation for each step of the process.
(a) The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide.
(b) The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water.
(c) Solid calcium hydroxide is then added to the seawater, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride.
(d) The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.
(e) Finally, the magnesium chloride is melted and electrolyzed to yield liquid liquid magnesium metal and diatomic chlorine gas.

Answer

(a) $\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$
(b) $\operatorname{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s)$
(c) $\mathrm{Ca}(\mathrm{OH})_{2}(s)+\mathrm{MgCl}_{2}(a q) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(s)+\mathrm{CaCl}_{2}(a q)$
(d) $\mathrm{Mg}(\mathrm{OH})_{2}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)$
(e) $\mathrm{MgCl}_{2}(l) \longrightarrow \mathrm{Mg}(l)+\mathrm{Cl}_{2}(g)$

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Video Transcript

for this question, you're given words to describe a chemical reaction and you're asked to write the balanced chemical reaction first. We have solid calcium carbonate, calcium has a two plus charge. Carbonate has a tu minus charge. So we need one carbonate for every calcium is going to decompose. And in the process produced solid calcium oxide. Again calcium two plus oxide to minus. So we just need one of each of them and gaseous carbon dioxide. And it is balanced as is one carbon one carbon one calcium one calcium three oxygen's three oxygen's than for part C. We have gaseous no we have solid aluminum metal that reacts with solid die atomic iodine. Sorry, wrong problem. We have solid calcium oxide that reacts with water in order to produce the product. Solid calcium hydroxide, calcium has the two plus charge. Hydroxide has a one minus charge. So we're going to need to hydroxide for every calcium. And this is balanced as is one calcium. One calcium to hydrogen is to hydrogen 12 oxygen's to oxygen's in the next step, solid calcium hydroxide, what we just determined up here is added to seawater reacting with magnesium chloride, acquis magnesium as the two plus charge, chloride has a one minus charge. So we need to chlorides for every magnesium. Then when the cat eye and switch places will end up with magnesium hydroxide. Magnesium with the two plus hydroxide with one minus requires two hydroxide for each magnesium and calcium chloride, calcium has a two plus charge chloride has a one minus charge. So we need to chlorides for every calcium and this is also balanced. No coefficients are needed. Then we have the magnesium hydroxide solid created here reacting with hydrochloric acid to produce magnesium chloride, magnesium chloride. We'll have to chlorides for every magnesium due to magnesium having a two plus charge in chloride having a one minus charge and liquid water. This one does need a coefficient because we have two chlorides here, we just had ones, we need to put it to in front of the hcl. This is going to give us 1234 hydrogen atoms and then we have 12 oxygen. And once we put it to here to get four hydrogen is, we'll have to oxygen's and then we have magnesium chloride decomposing with a high amount of energy into magnesium liquid and chlorine gas. And this is already balanced.

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