Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 22: Problem 70

Write a balanced equation for each of the following reactions: (a) Burning magnesium metal in a carbon dioxide atmosphere reduces the \(\mathrm{CO}_{2}\) to carbon. (b) In photosynthesis, solar energy is used to produce glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) and \(\mathrm{O}_{2}\) from carbon dioxide and water. (c) When carbonate salts dissolve in water, they produce basic solutions.

Short Answer

Expert verified
The short answer to the question is as follows: (a) \(2\textnormal{Mg} + \textnormal{CO}_2 \to 2\textnormal{MgO} + \textnormal{C}\) (b) \(6\textnormal{CO}_2 + 6\textnormal{H}_2\textnormal{O} \to \textnormal{C}_6\textnormal{H}_{12}\textnormal{O}_6 + 6\textnormal{O}_2\) (c) \(\textnormal{Na}_2\textnormal{CO}_3 + \textnormal{H}_2\textnormal{O} \to 2\textnormal{NaOH} + \textnormal{H}_2\textnormal{CO}_3\)

Step by step solution

01

Identify the reactants and products

In this reaction, magnesium (Mg) reacts with carbon dioxide (CO2) to produce magnesium oxide (MgO) and carbon (C).
02

Write the unbalanced equation

The unbalanced equation for this reaction is: Mg + CO2 -> MgO + C
03

Balance the equation

To balance the equation, we need to make sure the number of atoms for each element is equal on both sides of the equation. Mg + CO2 -> MgO + C 2Mg + CO2 -> 2MgO + C The balanced equation is: \(2\textnormal{Mg} + \textnormal{CO}_2 \to 2\textnormal{MgO} + \textnormal{C}\) #b) Photosynthesis (producing glucose and O2 from CO2 and H2O)#
04

Identify the reactants and products

In this reaction, carbon dioxide (CO2) and water (H2O) react under sunlight to produce glucose (C6H12O6) and oxygen (O2) gas.
05

Write the unbalanced equation

The unbalanced equation for this reaction is: CO2 + H2O -> C6H12O6 + O2
06

Balance the equation

To balance the equation, we need to make sure the number of atoms for each element is equal on both sides of the equation. 6CO2 + 6H2O -> C6H12O6 + 6O2 The balanced equation is: \(6\textnormal{CO}_2 + 6\textnormal{H}_2\textnormal{O} \to \textnormal{C}_6\textnormal{H}_{12}\textnormal{O}_6 + 6\textnormal{O}_2\) #c) Dissolution of carbonate salts in water to produce basic solutions#
07

Identify the reactants and products

In this reaction, we can use sodium carbonate (Na2CO3) as an example of a carbonate salt. It reacts with water (H2O) to produce sodium hydroxide (NaOH) and carbonic acid (H2CO3).
08

Write the unbalanced equation

The unbalanced equation for this reaction is: Na2CO3 + H2O -> NaOH + H2CO3
09

Balance the equation

To balance the equation, we need to make sure the number of atoms for each element is equal on both sides of the equation. Na2CO3 + H2O -> 2NaOH + H2CO3 The balanced equation is: \(\textnormal{Na}_2\textnormal{CO}_3 + \textnormal{H}_2\textnormal{O} \to 2\textnormal{NaOH} + \textnormal{H}_2\textnormal{CO}_3\)

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!

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

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium nitrite, (b) ammonia, (c) nitrous oxide, (d) sodium cyanide, (e) nitric acid, (f) nitrogen dioxide, (g) nitrogen, (h) boron nitride.

The solubility of \(\mathrm{Cl}_{2}\) in \(100 \mathrm{~g}\) of water at \(\mathrm{STP}\) is \(310 \mathrm{~cm}^{3}\). Assume that this quantity of \(\mathrm{Cl}_{2}\) is dissolved and equilibrated as follows: $$ \mathrm{Cl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Cl}^{-}(a q)+\mathrm{HClO}(a q)+\mathrm{H}^{+}(a q) $$ (a) If the equilibrium constant for this reaction is \(4.7 \times 10^{-4}\), calculate the equilibrium concentration of \(\mathrm{HClO}\) formed. \((\mathbf{b})\) What is the \(\mathrm{pH}\) of the final solution?

One method proposed for removing \(\mathrm{SO}_{2}\) from the flue gases of power plants involves reaction with aqueous \(\mathrm{H}_{2} \mathrm{~S}\). Elemental sulfur is the product. (a) Write a balanced chemical equation for the reaction. (b) What volume of \(\mathrm{H}_{2} \mathrm{~S}\) at \(27^{\circ} \mathrm{C}\) and 760 torr would be required to remove the \(\mathrm{SO}_{2}\) formed by burning 2.0 tons of coal containing \(3.5 \% \mathrm{~S}\) by mass? (c) What mass of elemental sulfur is produced? Assume that all reactions are \(100 \%\) efficient.

When ammonium perchlorate decomposes thermally, the products of the reaction are \(\mathrm{N}_{2}(g), \mathrm{O}_{2}(g), \mathrm{H}_{2} \mathrm{O}(g),\) and \(\mathrm{HCl}(g)\) (a) Write a balanced equation for the reaction. [Hint: You might find it easier to use fractional coefficients for the products.] (b) Calculate the enthalpy change in the reaction per mole of \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\). The standard enthalpy of formation of \(\mathrm{NH}_{4} \mathrm{ClO}_{4}(s)\) is \(-295.8 \mathrm{~kJ}\) (c) When \(\mathrm{NH}_{4} \mathrm{ClO}_{4}(s)\) is employed in solid-fuel booster rockets, it is packed with powdered aluminum. Given the high temperature needed for \(\mathrm{NH}_{4} \mathrm{ClO}_{4}(s)\) decomposition and what the products of the reaction are, what role does the aluminum play? (d) Calculate the volume of all the gases that would be produced at STP, assuming complete reaction of one pound of ammonium perchlorate.

Complete and balance the following equations: (a) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow\) (c) \(\mathrm{MnO}_{2}(s)+\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{AlP}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (e) \(\mathrm{Na}_{2} \mathrm{~S}(s)+\mathrm{HCl}(a q) \longrightarrow\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

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