/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 26 Describe 1 mole of \(\mathrm{CO}... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 5: Problem 26

Describe 1 mole of \(\mathrm{CO}_{2}\) in as many ways as you can.

Short Answer

Expert verified
1 mole of \(\mathrm{CO}_{2}\) contains \(6.022\times10^{23}\) molecules, has a molecular composition of \(6.022\times10^{23}\) carbon atoms and \(2\times(6.022\times10^{23})\) oxygen atoms, and has a mass of 44 grams. At STP, it occupies a volume of 22.4 liters with a density of approximately \(1.964\) g/L. Its standard enthalpy of formation is \( -393.5 \) kJ/mol, and it participates in various chemical reactions, such as photosynthesis, where it reacts with water to form glucose and oxygen gas.

Step by step solution

01

1. Define a mole in terms of particles

A mole is the unit of measurement in chemistry that represents \(6.022\times10^{23}\) particles of a substance. In this case, 1 mole of \(\mathrm{CO}_{2}\) contains \(6.022\times10^{23}\) molecules of carbon dioxide.
02

2. Molecular composition

Each molecule of carbon dioxide (\( \mathrm{CO}_{2} \)) is composed of one carbon atom (C) and two oxygen atoms (O). So, in 1 mole of \(\mathrm{CO}_{2}\), there are \( 6.022\times10^{23} \) carbon atoms and \( 2\times(6.022\times10^{23}) \) oxygen atoms.
03

3. Molar mass

The molar mass of \(\mathrm{CO}_{2}\) can be calculated using the atomic masses of carbon and oxygen. The atomic mass of carbon is approximately 12 grams per mole, and the atomic mass of oxygen is approximately 16 grams per mole. Thus, the molar mass of \(\mathrm{CO}_{2}\) is \(12 + 2\times16=44 \) grams per mole. So, 1 mole of \(\mathrm{CO}_{2}\) has a mass of 44 grams.
04

4. Volume at STP

At standard temperature and pressure (STP), which is defined as 0掳C (273.15 K) and 1 atmosphere (atm) pressure, the volume of 1 mole of any ideal gas is equal to 22.4 liters. Therefore, at STP, 1 mole of \(\mathrm{CO}_{2}\) occupies a volume of 22.4 liters.
05

5. Density at STP

The density of a substance can be calculated using the formula: density = mass/volume. At STP, the mass of 1 mole of \(\mathrm{CO}_{2}\) is 44 grams and the volume is 22.4 liters. Therefore, the density of 1 mole of \(\mathrm{CO}_{2}\) at STP is \( \frac{44 \text{g}}{22.4 \text{L}} \approx 1.964 \) g/L.
06

6. Partial pressure

The partial pressure of \(\mathrm{CO}_{2}\) in a gas mixture can be determined using Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of all the individual gases. If we know the total pressure and the mole fraction (concentration) of \(\mathrm{CO}_{2}\) in the mixture, we can calculate its partial pressure.
07

7. Energy content

The energy content of \(\mathrm{CO}_{2}\) can be described in terms of its enthalpy of formation, which is the heat released or absorbed when 1 mole of a compound is formed from its constituent elements under standard conditions. The standard enthalpy of formation of \(\mathrm{CO}_{2}\) is \( -393.5 \) kJ/mol, meaning that 393.5 kJ of heat is released when 1 mole of \(\mathrm{CO}_{2}\) is formed from its elements.
08

8. Chemical reactions involving \(\mathrm{CO}_{2}\)

One mole of \(\mathrm{CO}_{2}\) can also be described in terms of the chemical reactions it participates in. For example, during photosynthesis, 1 mole of \(\mathrm{CO}_{2}\) reacts with 1 mole of water (H鈧侽) to produce 1 mole of glucose (C鈧咹鈧佲倐O鈧�) and 6 moles of oxygen (O鈧�) gas. In this case, the balanced chemical equation for photosynthesis is: \( \mathrm{CO}_{2} + \mathrm{H}_{2}\mathrm{O} \rightarrow \mathrm{C}_{6}\mathrm{H}_{12}\mathrm{O}_{6} + \mathrm{O}_{2} \).

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

Consider samples of phosphine \(\left(\mathrm{PH}_{3}\right),\) water \(\left(\mathrm{H}_{2} \mathrm{O}\right),\) hydrogen sulfide \(\left(\mathrm{H}_{2} \mathrm{S}\right),\) and hydrogen fluoride (HF), each with a mass of \(119 \mathrm{g} .\) Rank the compounds from the least to the greatest number of hydrogen atoms contained in the samples.

A compound that contains only carbon, hydrogen, and oxygen is \(48.64 \%\) C and \(8.16 \%\) H by mass. What is the empirical formula of this substance?

With the advent of techniques such as scanning tunneling microscopy, it is now possible to "write" with individual atoms by manipulating and arranging atoms on an atomic surface. a. If an image is prepared by manipulating iron atoms and their total mass is \(1.05 \times 10^{-20} \mathrm{g},\) what number of iron atoms were used? b. If the image is prepared on a platinum surface that is exactly 20 platinum atoms high and 14 platinum atoms wide, what is the mass (grams) of the atomic surface? c. If the atomic surface were changed to ruthenium atoms and the same surface mass as determined in part b is used, what number of ruthenium atoms is needed to construct the surface?

Boron consists of two isotopes, \(^{10} \mathbf{B}\) and \(^{11} \mathbf{B}\). Chlorine also has two isotopes, \(^{35} \mathrm{Cl}\) and \(^{37} \mathrm{Cl}\). Consider the mass spectrum of \(\mathrm{BCl}_{3}\) How many peaks would be present, and what approximate mass would each peak correspond to in the \(\mathrm{BCl}_{3}\) mass spectrum?

Arrange the following substances in order of increasing mass percent of carbon. a. caffeine, \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{N}_{4} \mathrm{O}_{2}\) b. sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) c. ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Analysis

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.