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Chapter 6: Problem 31

Calcium oxide is sometimes very challenging to store in the chemistry laboratory. This compound reacts with moisture in the air and is converted to calcium hydroxide. If a bottle of calcium oxide is left on the shelf too long, it gradually absorbs moisture from the humidity in the laboratory. Eventually the bottle cracks and spills the calcium hydroxide that has been produced. Write the unbalanced chemical equation for this process.

Short Answer

Expert verified
The unbalanced chemical equation for the reaction between calcium oxide (CaO) and moisture (H2O) to form calcium hydroxide (Ca(OH)2) is: CaO + H2O → Ca(OH)2

Step by step solution

01

Identify the reactants

In this process, calcium oxide (CaO) reacts with moisture, which is water (H2O), from the air.
02

Write the reactants

Write down the reactants involved in the process: CaO + H2O
03

Identify the product

The process results in the formation of calcium hydroxide (Ca(OH)2).
04

Write the product

Write down the product formed in the process: → Ca(OH)2
05

Combine reactants and product to form the unbalanced equation

Combine the reactants and the product to write the unbalanced chemical equation: CaO + H2O → Ca(OH)2

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Most popular questions from this chapter

Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach,producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a "burp"). Write the unbalanced chemical equation for this process.

The Group 2 metals\((\mathrm{Ba}, \mathrm{Ca}, \mathrm{Sr})\) can be produced in the elemental state by the reaction of their oxides with aluminum metal at high temperatures, also producing solid aluminum oxide as a by-product. Write the unbalanced chemical equations for the reactions of barium oxide, calcium oxide, and strontium oxide with aluminum.

Balance each of the following chemical equations. a. \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{CrO}_{4}(a q) \rightarrow\) \(\mathrm{BaCrO}_{4}(s)+\mathrm{NaNO}_{3}(a q)\) b. \(\operatorname{PbCl}_{2}(a q)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q) \rightarrow \operatorname{PbSO}_{4}(s)+\mathrm{KCl}(a q)\) c. \(C_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{CaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s)+\mathrm{C}_{2} \mathrm{H}_{2}(g)\) e. \(\operatorname{Sr}(s)+\operatorname{HNO}_{3}(a q) \rightarrow \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2}(g)\) f. \(\mathrm{BaO}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)\) g. \(A s I_{3}(s) \rightarrow A s(s)+I_{2}(s)\) h. \(\operatorname{CuSO}_{4}(a q)+\mathrm{KI}(s) \rightarrow \operatorname{CuI}(s)+\mathrm{I}_{2}(s)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)\)

How do we indicate the physical state of a substance when we write a chemical equation for a reaction?

Hydrogen sulfide gas is responsible for the odor of rotten eggs. Hydrogen sulfide burns in air, producing sulfur dioxide gas and water vapor. Write the unbalanced chemical equation for this process.
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