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Chapter 21: Problem 88

Complete and balance the following. Write the simplest equation possible. If no reaction occurs, so state. (a) \(\operatorname{Li}_{2} \mathrm{CO}_{3}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow}\) (b) \(\mathrm{CaCO}_{3}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \longrightarrow\) (c) \(\mathrm{Al}(\mathrm{s})+\mathrm{NaOH}(\mathrm{aq}) \longrightarrow\) (d) \(\operatorname{BaO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\) (e) \(\mathrm{Na}_{2} \mathrm{O}_{2}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g}) \longrightarrow\)

Short Answer

Expert verified
The balanced equations are: (a) \(Li_2CO_3 \stackrel{\Delta}{\longrightarrow} Li_2O + CO_2\), (b) \(CaCO_3 + 2HCl \longrightarrow CaCl_2 + H_2O + CO_2\), (c) \(2Al + 2NaOH + 6H_2O \longrightarrow 2Na[Al(OH)_4]\), (d) \(BaO + H_2O \longrightarrow Ba(OH)_2\), (e) \(2Na_2O_2 + 2CO_2 \longrightarrow 2Na_2CO_3 + O_2\).

Step by step solution

01

Identify The Type of Reaction and The Possible Chemical Products

Looking at the reactants, we can identify the type of the reaction and potential products. By following established chemistry rules, it is possible to predict the products for each reaction. For example, a salt (like lithium carbonate) when exposed to heat (indicated by the delta symbol) generally undergoes decomposition, resulting in the formation of a metal oxide and carbon dioxide. The application of such reasoning would generate potential chemical products for each reaction.
02

Write The Unbalanced Chemical Equation

After predicting the products, write down the chemical reaction using the formula of these products. In each equation, the reactants will yield the predicted products.
03

Balance The Chemical Equation

Each equation must follow the Law of Conservation of Mass, meaning the number of atoms of each element must be the same on both the reactant and product sides of the equation. This step requires making sure that the equation is balanced by adjusting the coefficients in front of the chemical formulas.
04

Repeat The Process for Each Reaction

Repeat these steps for each of the chemical reactions mentioned in the exercise (a to e).

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Most popular questions from this chapter

Briefly describe each of the following ideas, methods, or phenomena: (a) diagonal relationship; (b) preparation of deionized water by ion exchange; (c) thermite reaction; (d) inert pair effect.

Write plausible chemical equations for preparing each compound from the indicated starting material: (a) \(\operatorname{SnCl}_{2}\) from \(\operatorname{SnO} ;\) (b) \(\operatorname{SnCl}_{4}\) from \(\operatorname{Sn} ;\) (c) \(\operatorname{PbCrO}_{4}\) from \(\mathrm{PbO}_{2}\). What reagents (acids, bases, salts) and equipment commonly available in the laboratory are needed for each reaction?

The molecule tetraborane has the formula \(\mathrm{B}_{4} \mathrm{H}_{10}\) (a) Show that this is an electron-deficient molecule. (b) How many bridge bonds must occur in the molecule? (c) Show that butane, \(\mathrm{C}_{4} \mathrm{H}_{10},\) is not electron deficient.

Write the simplest chemical equation to represent the reaction of (a) \(\mathrm{K}_{2} \mathrm{CO}_{3}\left(\text { aq) and } \mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq})\right.\); (b) \(\operatorname{Mg}\left(\mathrm{HCO}_{3}\right)_{2}(\) aq) on heating; (c) tin(II) oxide when heated with carbon; (d) \(\mathrm{CaF}_{2}(\mathrm{s})\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{concd}\) aq); (e) \(\mathrm{NaHCO}_{3}(\mathrm{s})\) and \(\mathrm{HCl}(\mathrm{aq}) ;\) (f) \(\mathrm{PbO}_{2}(\mathrm{s})\) and HBr(aq); and (g) the reduction of \(\mathrm{SiF}_{4}\) to pure \(\mathrm{Si},\) by using Na as the reducing agent.

Write chemical equations for the reactions you would expect to occur when (a) \(\operatorname{Mg}\left(\mathrm{HCO}_{3}\right)_{2}(\mathrm{s})\) is heated to a high temperature (b) \(\mathrm{BaCl}_{2}(1)\) is electrolyzed (c) \(\operatorname{Sr}(\text { s) is added to cold dilute } \operatorname{HBr}( \text { aq) }\) (d) \(\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq})\) is added to \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\) (e) \(\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\) is heated
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