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Chapter 7: Problem 78

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Chlorine reacts with water. (b) Barium metal is heated in an atmosphere of hydrogen gas. (c) Lithium reacts with sulfur. (d) Fluorine reacts with magnesium metal.

Short Answer

Expert verified
(a) Cl2 + H2O -> 2HClO + 2HCl (b) Ba + H2 -> BaH2 (c) 2Li + S -> Li2S (d) F2 + Mg -> MgF2

Step by step solution

01

Identify reactants and products

For this reaction, the reactants are chlorine (Cl2) and water (H2O). The products are hypochlorous acid (HClO) and hydrochloric acid (HCl).
02

Write the unbalanced chemical equation

Now, we can write down the unbalanced equation using the reactants and products. Cl2 + H2O -> HClO + HCl
03

Balance the equation

In order to balance the equation, we need to ensure the number of atoms for each element is the same on both sides of the equation. We can start by balancing the chlorine atoms. Since there are two chlorine atoms in Cl2 molecule and 1 in HCl and 1 in HClO, we need to have 2 molecules of HClO and 2 molecules of HCl: Cl2 + H2O -> 2HClO + 2HCl Now, the equation is balanced. (b) Barium metal is heated in an atmosphere of hydrogen gas
04

Identify reactants and products

For this reaction, the reactants are barium metal (Ba) and hydrogen gas (H2). The product is barium hydride (BaH2).
05

Write the unbalanced chemical equation

Now, we can write down the unbalanced equation using the reactants and products. Ba + H2 -> BaH2
06

Balance the equation

In order to balance the equation, we need to ensure the number of atoms for each element is the same on both sides of the equation. In this case, the equation is already balanced. (c) Lithium reacts with sulfur
07

Identify reactants and products

For this reaction, the reactants are lithium (Li) and sulfur (S). The product is lithium sulfide (Li2S).
08

Write the unbalanced chemical equation

Now, we can write down the unbalanced equation using the reactants and products. Li + S -> Li2S
09

Balance the equation

In order to balance the equation, we need to ensure the number of atoms for each element is the same on both sides of the equation. Since there are two lithium atoms in the Li2S molecule, we need to have 2 Li atoms on the reactant side: 2Li + S -> Li2S Now, the equation is balanced. (d) Fluorine reacts with magnesium metal
10

Identify reactants and products

For this reaction, the reactants are fluorine (F2) and magnesium (Mg). The product is magnesium fluoride (MgF2).
11

Write the unbalanced chemical equation

Now, we can write down the unbalanced equation using the reactants and products. F2 + Mg -> MgF2
12

Balance the equation

In order to balance the equation, we need to ensure the number of atoms for each element is the same on both sides of the equation. In this case, the equation is already balanced.

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Most popular questions from this chapter

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7}\). (a) What is the name of this product (see Table \(2.6\) )? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Under usual conditions, \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is a colorless liquid with a boiling point of \(81^{\circ} \mathrm{C}\). Is this boiling point expected or surprising? (d) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q)\) ? (e) If the oxygen in \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is considered to have the \(-2\) oxidation state, what is the oxidation state of the \(\mathrm{Cl}\) ? What is the electron configuration of \(\mathrm{Cl}\) in this oxidation state?

We will see in Chapter 12 that semiconductors are materials that conduct electricity better than nonmetals but not as well as metals. The only two elements in the periodic table that are technologically useful semiconductors are silicon and germanium. Integrated circuits in computer chips today are based on silicon. Compound semiconductors are also used in the electronics industry. Examples are gallium arsenide, GaAs; gallium phosphide, GaP; cadmium sulfide, CdS; and cadmium selenide, CdSe. (a) What is the relationship between the compound semiconductors' compositions and the positions of their elements on the periodic table relative to \(\mathrm{Si}\) and \(\mathrm{Ge}\) ? (b) Workers in the semiconductor industry refer to "II-VI" and "III-V" materials, using Roman numerals. Can you identify which compound semiconductors are II-VI and which are III-V? (c) Suggest other compositions of compound semiconductors based on the positions of their elements in the periodic table.

Potassium superoxide, \(\mathrm{KO}_{2}\), is often used in oxygen masks (such as those used by firefighters) because \(\mathrm{KO}_{2}\) reacts with \(\mathrm{CO}_{2}\) to release molecular oxygen. Experiments indicate that \(2 \mathrm{~mol}\) of \(\mathrm{KO}_{2}(s)\) react with each mole of \(\mathrm{CO}_{2}(g)\). (a) The products of the reaction are \(\mathrm{K}_{2} \mathrm{CO}_{3}(s)\) and \(\mathrm{O}_{2}(g)\). Write a balanced equation for the reaction between \(\mathrm{KO}_{2}(s)\) and \(\mathrm{CO}_{2}(g)\). (b) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced? (c) What mass of \(\mathrm{KO}_{2}(s)\) is needed to consume \(18.0 \mathrm{~g} \mathrm{CO}_{2}(\mathrm{~g})\) ? What mass of \(\mathrm{O}_{2}(g)\) is produced during this reaction?

Compare the elements bromine and chlorine with respect to the following properties: (a) electron configuration, (b) most common ionic charge, (c) first ionization energy, (d) reactivity toward water, (e) electron affinity, (f) atomic radius. Account for the differences between the two elements.

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.
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