Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

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) \(Cl_2 + H_2O \rightarrow HCl + HOCl\) b) \(Ba + 2H_2 \rightarrow BaH_2\) c) \(2Li + S \rightarrow Li_2S\) d) \(F_2 + Mg \rightarrow MgF_2\)

Step by step solution

01

a) Chlorine reacts with water

Chlorine (Cl2) reacts with water (H2O) to form hydrochloric acid (HCl) and hypochlorous acid (HOCl). The unbalanced equation is: Cl2 + H2O -> HCl + HOCl To balance the equation, we must make sure that the number of each type of atom on both the reactant and product side is equal. First, balance the chlorine atoms: 1 Cl2 (reactant side) = 1 HCl + 1 HOCl (product side) So, the chlorine atoms are already balanced. Next, balance the hydrogen and oxygen atoms: 1 H2O (reactant side) = 1 HCl + 1 HOCl (product side) So, the hydrogen and oxygen atoms are also balanced. Therefore, the balanced chemical equation is: Cl2 + H2O -> HCl + HOCl
02

b) Barium metal is heated in an atmosphere of hydrogen gas

Barium metal (Ba) reacts with hydrogen gas (H2) to form barium hydride (BaH2). The unbalanced equation is: Ba + H2 -> BaH2 To balance the equation, make sure that the number of each type of atom on both the reactant and product side is equal. First, balance the Barium atoms: 1 Ba (reactant side) = 1 Ba (product side) So, the Barium atoms are already balanced. Next, balance the Hydrogen atoms: 1 H2 (reactant side) = 2 H (product side) Therefore, we need to multiply the reactant H2 by 2. So, the balanced chemical equation is: Ba + 2H2 -> BaH2
03

c) Lithium reacts with sulfur

Lithium (Li) reacts with sulfur (S) to form lithium sulfide (Li2S). The unbalanced equation is: Li + S -> Li2S To balance the equation, make sure that the number of each type of atom on both the reactant and product side is equal. First, balance the Lithium atoms: 1 Li (reactant side) ≠ 2 Li (product side) So, we need to multiply the reactant Li by 2: 2Li + S -> Li2S Now, balance the sulfur atoms: 1 S (reactant side) = 1 S (product side) So, the sulfur atoms are already balanced, and our balanced chemical equation is: 2Li + S -> Li2S
04

d) Fluorine reacts with magnesium metal

Fluorine (F2) reacts with magnesium metal (Mg) to form magnesium fluoride (MgF2). The unbalanced equation is: F2 + Mg -> MgF2 To balance the equation, make sure that the number of each type of atom on both the reactant and product side is equal. First, balance the Magnesium atoms: 1 Mg (reactant side) = 1 Mg (product side) So, the Magnesium atoms are already balanced. Next, balance the Fluorine atoms: 2 F (reactant side) = 2 F (product side) So, the Fluorine atoms are also balanced. Therefore, the balanced chemical equation is: F2 + Mg -> MgF2

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Stoichiometry
Stoichiometry is a section of chemistry that involves calculating the relative quantities of reactants and products in chemical reactions. It is a critical component for scientists and engineers to ensure that reactions proceed with the desired efficiency and yield.

The heart of stoichiometry lies in the balanced chemical equation. A balanced equation obeys the Law of Conservation of Mass, which states that mass cannot be created or destroyed in a chemical reaction. Thus, we must have the same number of each type of atom on both sides of the equation. For example, in the reaction where chlorine (Cl2) reacts with water (H2O) to form hydrochloric acid (HCl) and hypochlorous acid (HOCl), stoichiometry ensures that the elements involved in the reaction are conserved.

To improve understanding of stoichiometry:
  • Visualize the atomic changes using particle diagrams.
  • Practice with mole-to-mole conversions.
  • Work on exercises involving limiting reagents and theoretical yields.
By mastering stoichiometry, students can predict the outcomes of reactions, design syntheses, and operate in a way that supports sustainable chemical practices.
Chemical Reaction
A chemical reaction is a process that leads to the chemical transformation of one set of substances into another. Chemical reactions can be represented by chemical equations, which show the reactants transforming into products. They can be simple, such as the combination of lithium (Li) and sulfur (S) to form lithium sulfide (Li2S), or complex, involving multiple steps and intermediates.

Understanding chemical reactions involves recognizing the types of reactions, such as synthesis, decomposition, single-replacement, double-replacement, and combustion. In the given exercises, different types of reactions are presented: the reaction of fluorine (F2) with magnesium (Mg) to form magnesium fluoride (MgF2) is an example of a synthesis reaction.

For those seeking to grasp the concept more firmly:
  • Study various categories of chemical reactions.
  • Perform lab experiments to observe reactions firsthand.
  • Learn to identify the products formed based on reactant properties.
Experimentation and observation are invaluable for understanding how reactants are transformed during chemical reactions.
Chemical Equation Balancing
Balancing chemical equations is essential for accurately representing a chemical reaction. It involves adjusting the coefficients of the molecules to ensure that there are an equal number of each type of atom on both the reactant and product sides of the equation. This reflects the principle that matter is conserved in a chemical reaction.

In the provided example, the reaction between barium (Ba) and hydrogen gas (H2) to form barium hydride (BaH2) is initially unbalanced. Balancing it involves ensuring that the number of hydrogen atoms in the reactants equals that in the products, leading to the balanced equation: Ba + 2H2 -> BaH2.

To enhance understanding in chemical equation balancing:
  • Start by balancing the atoms of elements that appear only once on each side.
  • Balance polyatomic ions as a whole where possible.
  • Check your work by confirming that all atoms balance at the end.
Chemical equation balancing is a fundamental skill in chemistry, enabling accurate predictions about the quantities of substances produced in chemical reactions.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Give three examples of ions that have an electron configuration of \(n d^{6}(n=3,4,5, \ldots).\)

Zincin its \(2+\) oxidation state is an essential metal ion for life. \(\mathrm{Zn}^{2+}\) is found bound to many proteins that are involved in biological processes, but unfortunately \(\mathrm{Zn}^{2+}\) is hard to detect by common chemical methods. Therefore, scientists who are interested in studying \(\mathrm{Zn}^{2+}\) -containing proteins frequently substitute \(\mathrm{Cd}^{2+}\) for \(\mathrm{Zn}^{2+},\) since \(\mathrm{Cd}^{2+}\) is easier to detect. (a) On the basis of the properties of the elements and ions discussed in this chapter and their positions in the periodic table, describe the pros and cons of using \(\mathrm{Cd}^{2+}\) as a \(\mathrm{Zn}^{2+}\) substitute. (b) Proteins that speed up (catalyze) chemical reactions are called enzymes. Many enzymes are required for proper metabolic reactions in the body. One problem with using \(\mathrm{Cd}^{2+}\) to replace \(\mathrm{Zn}^{2+}\) in enzymes is that \(\mathrm{Cd}^{2+}\) substitution can decrease or even eliminate enzymatic activity. Can you suggest a different metal ion that might replace \(Z n^{2+}\) in enzymes instead of \(C d^{2+} ?\) Justify your answer.

Detailed calculations show that the value of \(Z_{\text { eff }}\) for the outermost electrons in Si and Cl atoms is \(4.29+\) and \(6.12+\) , respectively.(a) What value do you estimate for \(Z\) eff experienced by the outermost electron in both Si and Cl by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant? (b) What values do you estimate for \(Z_{\text { eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text { eff? }} ?(\mathbf{d})\) Which method of approximation more accurately accounts for the steady increase in \(Z_{\text { eff }}\) that occurs upon moving left to right across a period? (e) Predict \(Z_{\text { eff }}\) for a valence electron in \(\mathrm{P}\) , phosphorus, based on the calculations for Si and Cl.

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) Ti, Ba; (b) Ag, Cu; (c) Ge, Cl; (d) Pb, Sb.

Identify two ions that have the following ground-state electron configurations: \((\mathbf{a}) [\) Ar \(],(\mathbf{b})[\) Ar \(] 3 d^{5},(\mathbf{c})[\mathrm{Kr}] 5 s^{2} 4 d^{10}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free