Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 22

Although the alkali metal halides can be prepared directly from the elements, the far less expensive industrial route is treatment of the carbonate or hydroxide with aqueous hydrohalic acid (HX) followed by recrystallization. Balance the reaction between potassium carbonate and aqueous hydriodic acid.

Short Answer

Expert verified
The balanced equation is \( K_2CO_3 + 2HI \rightarrow 2KI + CO_2 + H_2O \).

Step by step solution

01

Identify the Reactants and Products

The reactants are potassium carbonate (\(K_2CO_3\)) and hydriodic acid (\(HI\)). The products will be potassium iodide (\(KI\)), carbon dioxide (\(CO_2\)), and water (\(H_2O\)).
02

Write the Unbalanced Equation

We begin by writing the chemical equation with the correct formulas:\[ K_2CO_3 + HI \rightarrow KI + CO_2 + H_2O \]
03

Balance Potassium (K) Atoms

There are 2 potassium (K) atoms in \(K_2CO_3\) and 1 in \(KI\). Therefore, we need 2 \(KI\):\[ K_2CO_3 + HI \rightarrow 2KI + CO_2 + H_2O \]
04

Balance Iodine (I) Atoms

We have 2 iodine (I) atoms in 2 \(KI\), so we need 2 \(HI\) to balance the iodine:\[ K_2CO_3 + 2HI \rightarrow 2KI + CO_2 + H_2O \]
05

Balance Hydrogen (H) and Oxygen (O) Atoms

Check the balance for hydrogen and oxygen atoms. On the product side, we have 1 \(H_2O\), which means 2 hydrogens (H) and 1 oxygen (O). Since the reactants already balance the oxygens (3 from \(CO_3\)) and hydrogens (2 from 2 \(HI\)), the equation is balanced.
06

Write the Balanced Equation

The final balanced equation is:\[ K_2CO_3 + 2HI \rightarrow 2KI + CO_2 + H_2O \]

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.

Reactants
In a chemical reaction, 'reactants' are the starting substances that react with each other. They are the ingredients needed to start the chemical process. For example, in the exercise, the reactants are potassium carbonate \(K_2CO_3\) and hydriodic acid \(HI\).
Reactants always undergo a transformation during the reaction to become new substances called products. They are typically listed on the left side of the chemical equation.
Understanding the nature of reactants helps us predict the kind of reaction that will take place.
Products
'Products' are the substances that are formed as a result of the chemical reaction. They come from the transformation of reactants.
In our balancing exercise, the products are potassium iodide \(KI\), carbon dioxide \(CO_2\), and water \(H_2O\).
Products are shown on the right side of the chemical equation. Knowing the products of a chemical reaction allows us to understand the chemical changes that occurred and the result of the reaction.
Balanced Chemical Equation
A 'balanced chemical equation' ensures that the number of atoms for each element is the same on both sides of the equation. This is essential because the Law of Conservation of Mass states that matter cannot be created or destroyed in a chemical reaction.
To balance the provided exercise, we started with the unbalanced equation: \( K_2CO_3 + HI \rightarrow KI + CO_2 + H_2O \).
We then adjusted coefficients to ensure the same number of each type of atom appeared on both sides:
  • Balanced potassium by adding a coefficient of 2 to \(KI\)
  • Balanced iodine by adding a coefficient of 2 to \(HI\)
  • Checked hydrogen and oxygen to confirm they balanced
  • The final balanced equation is \( K_2CO_3 + 2HI \rightarrow 2KI + CO_2 + H_2O \).
This method helps in correctly describing the reaction.
Stoichiometry
'Stoichiometry' is the area of chemistry that involves calculating the quantities of reactants and products in a chemical reaction. It helps in understanding how much of a reactant is required or how much of a product will be formed.
In our example, stoichiometry helps us understand the ratio of reactants to products, such as 1 mole of potassium carbonate reacting with 2 moles of hydriodic acid to produce 2 moles of potassium iodide, 1 mole of carbon dioxide, and 1 mole of water.
This helps in practical applications, such as determining the quantities needed for industrial processes or laboratory experiments.

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

Selenium tetrafluoride reacts with fluorine to form selenium hexafluoride. (a) Draw Lewis structures for both selenium fluorides, and predict any deviations from ideal bond angles. (b) Describe the change in orbital hybridization of the central Se during the reaction.

Unlike other Group \(2 \mathrm{~A}(2)\) metals, beryllium reacts like aluminum and zinc with concentrated aqueous base to release hydrogen gas and form oxoanions of formula \(\mathrm{M}(\mathrm{OH})_{4}^{n-}\). Write equations for the reactions of these three metals with \(\mathrm{NaOH}\).

Give the name and symbol or formula of a Group \(7 \mathrm{~A}(17)\) element or compound that fits each description or use: (a) Used in etching glass (b) Compound used in household bleach (c) Weakest hydrohalic acid (d) Element that is a liquid at room temperature (e) Organic chloride used to make PVC

Copper(II) hydrogen arsenite (CuHAsO \(_{3}\) ) is a green pigment once used in wallpaper. In damp conditions, mold metabolizes this compound to trimethylarsine \(\left[\left(\mathrm{CH}_{3}\right)_{3} \mathrm{As}\right],\) a highly toxic gas. (a) Calculate the mass percent of As in each compound. (b) How much CuHAsO must react to reach a toxic level in a room that measures \(12.35 \mathrm{~m} \times 7.52 \mathrm{~m} \times 2.98 \mathrm{~m}\) (arsenic is toxic at \(\left.0.50 \mathrm{mg} / \mathrm{m}^{3}\right) ?\)

The triatomic molecular ion \(\mathrm{H}_{3}^{+}\) was first detected and characterized by J. J. Thomson using mass spectrometry. Use the bond energy of \(\mathrm{H}_{2}(432 \mathrm{~kJ} / \mathrm{mol})\) and the proton affinity of \(\mathrm{H}_{2}\left(\mathrm{H}_{2}+\mathrm{H}^{+} \longrightarrow \mathrm{H}_{3}^{+} ; \Delta H=-337 \mathrm{~kJ} / \mathrm{mol}\right)\) to calculate the en thalpy of reaction for \(\mathrm{H}+\mathrm{H}+\mathrm{H}^{+} \longrightarrow \mathrm{H}_{3}^{+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation

Chemical Reactions

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