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Chapter 7: Problem 65

Write balanced equations for the following reactions: (a) barium oxide with water, (b) iron(II) oxide with perchloric acid, (c) sulfur trioxide with water, (d) carbon dioxide with aqueous sodium hydroxide.

Short Answer

Expert verified
Here are the balanced equations for each reaction: (a) Barium oxide with water: \( BaO + H_2O \rightarrow Ba(OH)_2 \) (b) Iron(II) oxide with perchloric acid: \( 2FeO + 2HClO_4 \rightarrow 2Fe(ClO_4)_2 + 2H_2O \) (c) Sulfur trioxide with water: \( SO_3 + H_2O \rightarrow H_2SO_4 \) (d) Carbon dioxide with aqueous sodium hydroxide: \( CO_2 + 2NaOH \rightarrow Na_2CO_3 + H_2O \)

Step by step solution

01

Reaction 1: Barium oxide with water

1. Identify reactants and products: Reactants: Barium oxide (BaO) and water (H鈧侽) Product: Barium hydroxide (Ba(OH)鈧�) 2. Write the unbalanced equation: BaO + H鈧侽 鈫� Ba(OH)鈧� 3. Balance the equation: BaO + H鈧侽 鈫� Ba(OH)鈧� (The equation is already balanced with 1:1:1 stoichiometry)
02

Reaction 2: Iron(II) oxide with perchloric acid

1. Identify reactants and products: Reactants: Iron(II) oxide (FeO) and perchloric acid (HClO鈧�) Products: Iron(II) perchlorate (Fe(ClO鈧�)鈧�) and water (H鈧侽) 2. Write the unbalanced equation: FeO + HClO鈧� 鈫� Fe(ClO鈧�)鈧� + H鈧侽 3. Balance the equation: 2FeO + 2HClO鈧� 鈫� 2Fe(ClO鈧�)鈧� + 2H鈧侽
03

Reaction 3: Sulfur trioxide with water

1. Identify reactants and products: Reactants: Sulfur trioxide (SO鈧�) and water (H鈧侽) Product: Sulfuric acid (H鈧係O鈧�) 2. Write the unbalanced equation: SO鈧� + H鈧侽 鈫� H鈧係O鈧� 3. Balance the equation: SO鈧� + H鈧侽 鈫� H鈧係O鈧� (The equation is already balanced with 1:1:1 stoichiometry)
04

Reaction 4: Carbon dioxide with aqueous sodium hydroxide

1. Identify reactants and products: Reactants: Carbon dioxide (CO鈧�) and aqueous sodium hydroxide (NaOH) Products: Sodium carbonate (Na鈧侰O鈧�) and water (H鈧侽) 2. Write the unbalanced equation: CO鈧� + NaOH 鈫� Na鈧侰O鈧� + H鈧侽 3. Balance the equation: CO鈧� + 2NaOH 鈫� Na鈧侰O鈧� + H鈧侽

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Most popular questions from this chapter

It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measure how well electricity is conducted by each of the elements to determine how "metallic" the elements are. On the basis of conductivity, there is not much of a trend in the periodic table: Silver is the most conductive metal, and manganese the least. Look up the first ionization energies of silver and manganese; which of these two elements would you call more metallic based on the way we define it in this book?

Explain the following variations in atomic or ionic radii: (a) \(\mathrm{I}^{-}>\mathrm{I}>\mathrm{I}^{+}\) (b) \(\mathrm{Ca}^{2+}>\mathrm{Mg}^{2+}>\mathrm{Be}^{2+}\) (c) \(\mathrm{Fe}>\mathrm{Fe}^{2+}>\mathrm{Fe}^{3+}\)

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water. (b) Strontium is added to water. (c) Sodium reacts with oxygen. (d) Calcium reacts with iodine.

Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen. (c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine. (d) The third ionization energy of manganese is greater than those of both chromium and iron.

If the electron affinity for an element is a negative number, does it mean that the anion of the element is more stable than the neutral atom? Explain.
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