Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 6, Problem 108RQ
Interpretation Introduction
Interpretation:
The reason behind the fact that “molecular oxygen and ozone protect us from harmful ultraviolet radiation” is to be explained.
Concept Introduction:
Ozone is a colorless gas present in the upper atmosphere. It is a molecule made of three oxygen atoms.
Ozone is continuously formed in the atmosphere through different processes with the help of sunlight.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
1. What is the greenhouse effect?
2. What is good about the greenhouse effect? (Give at least two reasons.)
3. What is the most important greenhouse gas in the troposphere?
[References]
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and wate are the
products. Using the enthalpies of combustion for C,H2 (-1300. kJ/mol), C2Hs (-1560. kJ/mol), and H2 (-286 kJ/mol), calculate AH for the reaction
C2H2 (g) + 2H2 (g) C2H (g)
AH=
kJ
Submit Answer
Try Another Version
1 item attempt remaining
Previous
Next
8:33 P
12/5/20
a
S 0 門
thing
The combustion of hydrogen gas releases 286kJ per mol of hydrogen. If 11.0 L of hydrogen at STP was burned to produce electricity, how long would it power a 100-watt (W) light bulb? Assume no energy is lost to the surroundings. (1W = 1 J/s)
Chapter 6 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 6 - Prob. 1PECh. 6 - Prob. 2PECh. 6 - When monitoring a reaction, the initial...Ch. 6 - Practice Exercise 6.4
A hall bearing at is...Ch. 6 - Prob. 5PECh. 6 - Silicon, used in computer chips, has a specific...Ch. 6 - Would the explosive reaction of hydrogen and...Ch. 6 - Practice Exercise 6.8
When ammonium nitrate is...Ch. 6 - An exothermic reaction is carried out at a...Ch. 6 - For an exothermic reaction that is conducted under...
Ch. 6 - Since it can be obtained in very high purity,...Ch. 6 - A 1.50 g sample of pure sucrose is burned in a...Ch. 6 - For the Analyzing and Solving Multi-Concept...Ch. 6 - Practice Exercise 6.14
The exact same procedure as...Ch. 6 - The combustion of methane can be represented by...Ch. 6 - Practice Exercise 6.16
What is the thermochemical...Ch. 6 - Two oxides of copper can be made from copper by...Ch. 6 - Consider the following thermochemical...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Ethanol, C2H5OH, is made industrially by the...Ch. 6 - Practice Exercise 6.21
The heat of combustion, ,...Ch. 6 - Practice Exercise 6.22
n-Octane, , has a standard...Ch. 6 - Write the thermochemical equation that would be...Ch. 6 - Write the thermochemical equation that would be...Ch. 6 - Use heats of formation data from Table 6.2 to...Ch. 6 - Write thermochemical equations corresponding to Hf...Ch. 6 - Calculate H for the following reactions:...Ch. 6 - Give definitions for (a) energy, (b) kinetic...Ch. 6 - Prob. 2RQCh. 6 - Prob. 3RQCh. 6 - 6.4 State the law of conservation of energy....Ch. 6 - 6.5 A pendulum such as a swinging chandelier...Ch. 6 - Prob. 6RQCh. 6 - 6.7 What is meant by the term chemical energy?
Ch. 6 - How does the potential energy change (increase,...Ch. 6 - What is the SI unit of energy? How much energy (in...Ch. 6 - 6.10 Why is hear considered a waste product in a...Ch. 6 - Prob. 11RQCh. 6 - 6.12 How is internal energy related to molecular...Ch. 6 - On a molecular level, how is thermal equilibrium...Ch. 6 - Consider the distribution of molecular kinetic...Ch. 6 - Suppose the temperature of an object is raised...Ch. 6 - A quart of boiling water will cause a more severe...Ch. 6 - Prob. 17RQCh. 6 - What is a state function? Give four examples that...Ch. 6 - How would you determine whether an experimental...Ch. 6 - 6.20 How can the state of a system be specified?
Ch. 6 - 6.21 What do the terms system and surroundings...Ch. 6 - What are the names of the thermal properties whose...Ch. 6 - 6.23 For samples with the same mass, which kind of...Ch. 6 - 6.24 How do heat capacity and specific hear...Ch. 6 - Prob. 25RQCh. 6 - 6.26 Suppose object A has twice the specific heat...Ch. 6 - In a certain chemical reaction, there is a...Ch. 6 - 6.28 What term do we use to describe a reaction...Ch. 6 - 6.29 What term is used to describe a reaction that...Ch. 6 - 6.30 When gasoline burns, it reacts with oxygen in...Ch. 6 - Write the equation that states the first law of...Ch. 6 - How are heat and work defined?Ch. 6 - Devise an example, similar to the one described in...Ch. 6 - 6.34 Why are heat and work not state functions?
Ch. 6 - When we measure the heat of combustion of glucose,...Ch. 6 - Consider the reaction...Ch. 6 - How is enthalpy defined?Ch. 6 - What is the sign of H for an endothermic change?Ch. 6 - 6.39 If the enthalpy of a system increases by 100...Ch. 6 - If a system containing gases expands and pushes...Ch. 6 - 6.41 Why do standard reference values for...Ch. 6 - What distinguishes a thermochemical equation from...Ch. 6 - Why are fractional coefficients permitted in a...Ch. 6 - 6.44 What fundamental fact about makes Hess’s law...Ch. 6 - 6.45 What two conditions must be met by a...Ch. 6 - Describe what must be done with the standard...Ch. 6 - What two additional thermochemical equations are...Ch. 6 - Peptides, small parts of proteins, contain...Ch. 6 - If a car increases its speed from 30 mph to 60...Ch. 6 - 6.50 If the mass of a truck is doubled—for...Ch. 6 - 6.51 What is the kinetic energy, in joules, of a...Ch. 6 - What is the kinetic energy, in joules, of a...Ch. 6 - How much heat, in joules and in calories, must be...Ch. 6 - 6.54 How much heat, in joules and calories, is...Ch. 6 - How many grams of water can be heated from...Ch. 6 - 6.56 How many grams of copper can be cooled from ...Ch. 6 - A 50.0 g piece of a metal at 100.0C was plunged...Ch. 6 - 6.58 A sample of copper was heated to and then...Ch. 6 - 6.59 Calculate the molar heat capacity of iron in...Ch. 6 - 6.60 What is the molar heat capacity of ethyl...Ch. 6 - A vat of 4.54 kg of water underwent a decrease in...Ch. 6 - A container filled with 2.46 kg of water underwent...Ch. 6 - 6.63 Nitric acid neutralizes potassium hydroxide....Ch. 6 - In the reaction between formic acid (HCHO2) and...Ch. 6 - 6.65 A 1.000 mol sample of propane, a gas used for...Ch. 6 - Toluene, C7H8, is used in the manufacture of...Ch. 6 - If a system does 4$ J of work and receives 28 J of...Ch. 6 - If a system has 48 J of work done on it and...Ch. 6 - An automobile engine converts heat into work via a...Ch. 6 - Chargers for cell phones get warm while they are...Ch. 6 - If the engine in Problem 6.69 absorbs 250 joules...Ch. 6 - If a battery can release 535 J of energy and 455 J...Ch. 6 - Ammonia reacts with oxygen as follows:...Ch. 6 - One thermochemical equation for the reaction of...Ch. 6 - Magnesium bums in air to produce a bright light...Ch. 6 - Methanol is the fuel in canned heat containers...Ch. 6 - Methane burns with oxygen to produce carbon...Ch. 6 - Methanol, as described in Problem 6.76, is used to...Ch. 6 - *6.79 Construct an enthalpy diagram that shows the...Ch. 6 - *6.80 Construct an enthalpy diagram for the...Ch. 6 - Show how the equations...Ch. 6 - 6.82 We can generate hydrogen chloride by heating...Ch. 6 - Calculate H in kilojoules for the following...Ch. 6 - Calcium hydroxide reacts with hydrochloric acid by...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - 6.86 Given the following thermochemical...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Which of the following thermochemical equations...Ch. 6 - Which of the following thermochemical equations...Ch. 6 - Write the thermochcmical equations, including...Ch. 6 - Write the thermochemical equations, including...Ch. 6 - Using data in Table 6.2, calculate H in kilojoules...Ch. 6 - 6.94 Using data in Table 6.2, calculate in...Ch. 6 - The value for the standard heat of combustion, H...Ch. 6 - The thermochemical equation for the combustion of...Ch. 6 - 6.97 Look at the list of substances in Table 6.1....Ch. 6 - *6.98 A dilute solution of hydrochloric acid with...Ch. 6 - A 2.00 kg piece of granite with a specific heat of...Ch. 6 - In the recovery of iron from iron ore, the...Ch. 6 - Use the results of Problem 6.100 and the data in...Ch. 6 - 6.102 The amino acid glycine, , is one of the...Ch. 6 - The value of Hf for HBr(g) was first evaluated...Ch. 6 - Acetylene, C2H2, is a gas commonly burned in...Ch. 6 - The reaction for the metabolism of sucrose,...Ch. 6 - Consider the following thermochemical...Ch. 6 - 6.107 Chlorofluoromethanes (CFMs) are carbon...Ch. 6 - Prob. 108RQCh. 6 - Suppose a truck with a mass of 14.0 tons...Ch. 6 - How much work must be done to form one mole of CH4...Ch. 6 - A cold -15C piece of copper metal weighing 7.38 g...Ch. 6 - Both Na2CO3 and NaHCO3 can be used to neutralize...Ch. 6 - *6.113 When 4.56 g of a solid mixture composed of ...Ch. 6 - Using the results from Analyzing and Solving...Ch. 6 - *6.115 For ethanol, , which is mixed with gasoline...Ch. 6 - Both calcium and potassium react with water to...Ch. 6 - 6.117 As a routine safety procedure, acids and...Ch. 6 - In an experiment, 95.0 mL of 0.225 M silver...Ch. 6 - 6.119 Growing wheat and converting it into bread...Ch. 6 - Suppose we compress a spring, tie it up tightly,...Ch. 6 - Prob. 121RQCh. 6 - Why do we usually use H rather than E when we...Ch. 6 - Prob. 123RQCh. 6 - 6.124 Find the heats of formation of some...Ch. 6 - Prob. 125RQ
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?arrow_forwardhat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?arrow_forward1. Draw Lewis structures for ozone and for dioxygen. Using the data given below, qualitatively compare the bond enthalpies, bond orders, and bond lengths of these two compounds. O₂ (g) 20 (g) AH" = +498 kJ O(g) + O₂(g) →O, (g) AH-105 kJarrow_forward
- What is the greenhouse effect? How does the excess CO2 gas in the atmosphere cause the greenhouse effect?arrow_forwardExplain the Greenhouse Effect: Global Warming and Climate Change.arrow_forwardWhat is the theoretical yield of ammonia (in grams) if 16.55 grams of nitrogen gas and 10.15 grams of hydrogen gas are allowed to react? The enthalpy of this reaction is 92.22 kj.arrow_forward
- what is the enthalpy change per mole of CO2 for the followingreaction?CO(g) + 1/2 O2(g) CO2(g)arrow_forwardIt is often said that water vapour amplifies the Earth’s greenhouse effect. Indicate one way that an increased atmospheric concentration water vapour can increase the greenhouse effect and one way that it can decrease the greenhouse effect.arrow_forward[References] Sulfur (2.67 g) was burned in a constant volume calorimeter with excess 0, (g). The temperature increased from 20.63 °C to 26.42 °C. The bomb has a heat capacity of 909 J/K, and the calorimeter contained 804 g of water. (Specific heat capacity of water is 4.184 J/g · K.) Calculate AU per mole of SO2 formed for the reaction. S8 (s) + 8 O2 (g) → 8 SO2 (g) Sulfur burns in oxygen with a bright blue flame to give SO2 (g). AU = kJ/mol Visitedarrow_forward
- If the enthalpy change for the reaction below is 46.72 kJ, how many grams of ammonia can be produced if 50.7 kJ of heat energy are provided to the reaction? 4 NO + 6 H2O --> 4 NH3 + 5 O2arrow_forwardIf the enthalpy change for the reaction below is 46.72 kJ, how many grams of ammonia canbe produced if 50.7 kJ of heat energy are provided to the reaction? 4 NO + 6 H2O --> 4 NH3 + 5 O2arrow_forwardGive two examples of reactions which are driven by enthalpy change.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning