Connect for Chemistry
13th Edition
ISBN: 9781260161854
Author: Raymond Chang, Jason Overby
Publisher: Mcgraw-hill Higher Education (us)
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 20, Problem 20.41QP
The molar heat capacity of a diatomic molecule is 29.1 J/K · mol. Assuming the atmosphere contains only nitrogen gas and there is no heat loss, calculate the total heat intake (in kilojoules) if the atmosphere warms up by 3°C during the next 50 yr. Given that there are 1.8 × 1020 moles of diatomic molecules present, how many kilograms of ice (at the North and South Poles) will this quantity of heat melt at 0°C? (The molar heat of fusion of ice is 6.01 kJ/mol.)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
The molar heat capacity of a diatomic molecule is 29.1 J/K · mol. Assuming the atmosphere contains
only nitrogen gas and there is no heat loss, calculate the total heat intake (in kJ) if the atmosphere
warms up by 3.0°C during the next 50 years. Given that there are 2.8 x 10²20 moles of diatomic molecule
present, how many kilograms of ice (at the North and South Poles) will this quantity of heat melt at 0°
C? (The molar heat of fusion of ice is 6.01 kJ/mol.)
Total heat intake:
× 10
kJ
Ice melted:
× 10
|kg
(Enter your answer in scientific notation.)
6CO2(g) + 6H2O(l) → C6H12O6(s) + 6O2(g) ΔH = +2803 kJ/mol Calculate the mass (in grams) of O2 that is produced by photosynthesis when
24300 kJ of solar energy is consumed. Put your answer in scientific notation.
The citizens of the world burn the fossil fuel equivalent of 7 * 1012 kg of petroleum per year. Assume that all of this petroleum is in the form of octane (C8H18) and calculate how much CO2 (in kg) the world produces from fossil fuel combustion per year. (Hint: Begin by writing a balanced equation for the combustion of octane.) If the atmosphere currently contains approximately3 * 1015 kg of CO2, how long will it take for the world’s fossil fuel combustion to double the amount of atmospheric carbon dioxide?
Chapter 20 Solutions
Connect for Chemistry
Ch. 20.2 - Calculate the wavelength (in nm) of a photon...Ch. 20.5 - Prob. 2PECh. 20.5 - Prob. 1RCFCh. 20.8 - Prob. 3PECh. 20 - Prob. 20.1QPCh. 20 - Prob. 20.2QPCh. 20 - Prob. 20.3QPCh. 20 - Prob. 20.4QPCh. 20 - Prob. 20.5QPCh. 20 - Prob. 20.6QP
Ch. 20 - Prob. 20.7QPCh. 20 - Prob. 20.8QPCh. 20 - Prob. 20.9QPCh. 20 - Prob. 20.10QPCh. 20 - Prob. 20.11QPCh. 20 - The green color observed in aurora borealis is...Ch. 20 - Prob. 20.13QPCh. 20 - Prob. 20.14QPCh. 20 - Prob. 20.15QPCh. 20 - Prob. 20.16QPCh. 20 - Prob. 20.17QPCh. 20 - Prob. 20.18QPCh. 20 - Prob. 20.19QPCh. 20 - Prob. 20.20QPCh. 20 - Prob. 20.21QPCh. 20 - Prob. 20.22QPCh. 20 - Prob. 20.23QPCh. 20 - Prob. 20.24QPCh. 20 - Prob. 20.25QPCh. 20 - Prob. 20.26QPCh. 20 - Prob. 20.27QPCh. 20 - Prob. 20.28QPCh. 20 - Prob. 20.29QPCh. 20 - Prob. 20.30QPCh. 20 - Prob. 20.31QPCh. 20 - Prob. 20.32QPCh. 20 - Prob. 20.33QPCh. 20 - Prob. 20.34QPCh. 20 - Prob. 20.35QPCh. 20 - Prob. 20.36QPCh. 20 - Prob. 20.37QPCh. 20 - Prob. 20.38QPCh. 20 - Prob. 20.39QPCh. 20 - Calcium oxide or quicklime (CaO) is used in...Ch. 20 - The molar heat capacity of a diatomic molecule is...Ch. 20 - Prob. 20.42QPCh. 20 - Prob. 20.43QPCh. 20 - List three detrimental effects of acid rain.Ch. 20 - Briefly discuss two industrial processes that lead...Ch. 20 - Discuss ways to curb acid rain.Ch. 20 - Prob. 20.47QPCh. 20 - Describe the removal of SO2 by CaO (to form CaSO3)...Ch. 20 - Prob. 20.49QPCh. 20 - Prob. 20.50QPCh. 20 - Prob. 20.51QPCh. 20 - Prob. 20.52QPCh. 20 - Identify the gas that is responsible for the brown...Ch. 20 - The safety limits of ozone and carbon monoxide are...Ch. 20 - Prob. 20.55QPCh. 20 - In which region of the atmosphere is ozone...Ch. 20 - Assume that the formation of nitrogen dioxide:...Ch. 20 - The gas-phase decomposition of peroxyacetyl...Ch. 20 - On a smoggy day in a certain city the ozone...Ch. 20 - Which of the following settings is the most...Ch. 20 - Prob. 20.61QPCh. 20 - Prob. 20.62QPCh. 20 - Prob. 20.63QPCh. 20 - Prob. 20.64QPCh. 20 - A concentration of 8.00 102 ppm by volume of CO...Ch. 20 - Prob. 20.66QPCh. 20 - Briefly describe the harmful effects of the...Ch. 20 - The equilibrium constant (KP) for the reaction is...Ch. 20 - As stated in the chapter, carbon monoxide has a...Ch. 20 - Instead of monitoring carbon dioxide, suggest...Ch. 20 - In 1991 it was discovered that nitrous oxide (N2O)...Ch. 20 - A glass of water initially at pH 7.0 is exposed to...Ch. 20 - A 14-m by 10-m by 3.0-m basement had a high radon...Ch. 20 - Ozone in the troposphere is formed by the...Ch. 20 - Prob. 20.75QPCh. 20 - Prob. 20.76QPCh. 20 - A person was found dead of carbon monoxide...Ch. 20 - The carbon dioxide level in the atmosphere today...Ch. 20 - What is funny about the following cartoon?Ch. 20 - Calculate the standard enthalpy of formation (Hf )...Ch. 20 - Prob. 20.81QPCh. 20 - Prob. 20.82QPCh. 20 - Prob. 20.83QPCh. 20 - Peroxyacetyl nitrate (PAN) undergoes thermal...Ch. 20 - How are past temperatures determined from ice...Ch. 20 - The balance between SO2 and SO3 is important in...Ch. 20 - Prob. 20.87QPCh. 20 - The HO3 radical was once thought of as a temporary...Ch. 20 - What is the difference between weather and...Ch. 20 - Estimate the annual production of carbon dioxide...
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
- Calcium carbide, CaC2, is manufactured by reducing lime with carbon at high temperature. (The carbide is used in turn to make acetylene, an industrially important organic chemical.) Is the reaction endothermic or exothermic?arrow_forwardExplain why oceanfront areas generally have smaller temperature fluctuations than inland areas.arrow_forward62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?arrow_forward
- Formic acid, HCHO2, was first discovered in ants (formica is Latin for ant). In an experiment, 5.48 g of formic add was burned at constant pressure. 2HCHO2(l)+O2(g)2CO2(g)+2H2O(l) If 30.3 kJ of heat evolved, what is H per mole of formic acid?arrow_forwardWhat is the biological importance of stratospheric ozone? Explain.arrow_forwardPropane, C3H8, is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for the complete combustion of propane gas. (b) Calculate the volume of air at 25 C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later chapter on gasesfor now use the information that 1.00 L of air at 25 C and 1.00 atm contains 0.275 g of 2 per liter.) (c) The heat of combustion of propane is 2,219.2 kJ/mol. Calculate the heat of formation, Hf of propane given that Hf of H2O(l)=285.8 kJ/mol and Hf of CO2(g)=393.5 kJ/mol. (d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.arrow_forward
- One of the components of polluted air is NO. It is formed in the high-temperature environment of internal combustion engines by the following reaction: N2(g)+O2(g)2NO(g)H=180KJ Why are high temperatures needed to convert N2 and O2 to NO?arrow_forwardWhy is it a good idea to rinse your thermos bottle with hot water before filling it with hot coffee?arrow_forwardAn industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?arrow_forward
- The Sun supplies about 1.0 kilowatt of energy for each squaremeter of surface area (1.0 kW/m2, where a watt = 1 J/s).Plants produce the equivalent of about 0.20 g of sucrose(C12H22O11) per hour per square meter. Assuming that thesucrose is produced as follows, calculate the percentage ofsunlight used to produce sucrose.12 CO2(g)+ 11 H2O(l)-----> C12H22O11 + 12 O2(g)ΔH = 5645 kJarrow_forwardThe flame in a torch used to cut metal is produced by burning acetylene (C2H2) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 90.8 × 104kJ of heat?arrow_forwardThe sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1 J/s). The plants in an agricultural field produce the equivalent of 23 kg of sucrose (C12H22 O11) per hour per hectare (1 ha = 10,000 m²). Assuming that sucrose is produced by the reaction 12CO₂(g) + 11H₂O(l) → C12H22 O11 (8) + 1202 (9) AH = 5640 kJ calculate the percentage of sunlight used to produce the sucrose - that is, determine the efficiency of photosynthesis in this field. Percent efficiency = %arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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
Types of Matter: Elements, Compounds and Mixtures; Author: Professor Dave Explains;https://www.youtube.com/watch?v=dggHWvFJ8Xs;License: Standard YouTube License, CC-BY