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Chapter 6: Problem 70

When copper(II) oxide is boiled in an aqueous solution of sulfuric acid, a strikingly blue solution of copper(II) sulfate forms along with additional water. Write the unbalanced chemical equation for this reaction.

Short Answer

Expert verified
The unbalanced chemical equation for the reaction between copper(II) oxide (CuO) and sulfuric acid (H₂SO₄) is: \( \text{CuO} + \text{H₂SO₄} \to \text{CuSO₄} + \text{H₂O} \)

Step by step solution

01

Identify Reactants and Products

The reactants in this reaction are copper(II) oxide (CuO) and sulfuric acid (H₂SO₄). During the reaction, a blue solution of copper(II) sulfate (CuSO₄) forms as a product, along with additional water (H₂O).
02

Write the Unbalanced Chemical Equation

Now that we know the reactants and products, we can write the unbalanced chemical equation for this reaction: \( \text{CuO} + \text{H₂SO₄} \to \text{CuSO₄} + \text{H₂O} \) This is the unbalanced chemical equation for the reaction between copper(II) oxide and sulfuric acid, and it shows that copper(II) sulfate and water are produced during the reaction.

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Most popular questions from this chapter

When solid red phosphorus, \(P_{4}\), is burned in air, the phosphorus combines with oxygen, producing a choking cloud of tetraphosphorus decoxide. Write the unbalanced chemical equation for this reaction.

In a chemical equation for a reaction, the notation \("(a q) "\) after a substance's formula means that the substance is dissolved in _________ .

Balance each of the following chemical equations. a. \(\mathrm{H}_{2} \mathrm{O}_{2}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) b. \(\mathrm{Ag}(s)+\mathrm{H}_{2} \mathrm{S}(g) \rightarrow \mathrm{Ag}_{2} \mathrm{S}(s)+\mathrm{H}_{2}(g)\) c. \(\operatorname{FeO}(s)+\mathrm{C}(s) \rightarrow \operatorname{Fe}(l)+\mathrm{CO}_{2}(g)\) d. \(\quad \mathrm{Cl}_{2}(g)+\mathrm{KI}(a q) \rightarrow \mathrm{KCl}(a q)+\mathrm{I}_{2}(s)\) e. \(\mathrm{Na}_{2} \mathrm{B}_{4} \mathrm{O}_{7}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow\) \(\mathrm{H}_{3} \mathrm{BO}_{3}(s)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) f. \(\mathrm{CaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s)+\mathrm{C}_{2} \mathrm{H}_{2}(g)\) g. \(\mathrm{NaCl}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(l) \rightarrow \mathrm{HCl}(g)+\mathrm{Na}_{2} \mathrm{SO}_{4}(s)\) h. \(\mathrm{SiO}_{2}(s)+\mathrm{C}(s) \rightarrow \mathrm{Si}(l)+\mathrm{CO}(g)\)

When iron wire is heated in the presence of sulfur, the iron soon begins to glow, and a chunky, blue black mass of iron(II) sulfide is formed. Write the unbalanced chemical equation for this reaction.

Balance each of the following chemical equations. a. \(\mathrm{FeCl}_{3}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{Fe}(\mathrm{OH})_{3}(s)+\mathrm{KCl}(a q)\). b. \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+\mathrm{KI}(a q) \rightarrow\) \(\mathrm{PbI}_{2}(s)+\mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) c. \(\mathrm{P}_{4} \mathrm{O}_{10}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)\) d. \(\mathrm{Li}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{LiOH}(a q)\) e. \(\operatorname{MnO}_{2}(s)+\mathrm{C}(s) \rightarrow \operatorname{Mn}(s)+\mathrm{CO}_{2}(g)\) f. \(\operatorname{Sb}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{SbCl}_{3}(s)\) g. \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) h. \(\operatorname{FeS}(s)+\operatorname{HCl}(a q) \rightarrow \operatorname{Fe} \mathrm{Cl}_{2}(a q)+\mathrm{H}_{2} \mathrm{S}(g)\)
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