Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 21, Problem 21.65QP
Interpretation Introduction
Interpretation: It should be explained the past temperature determination from ice cores obtained from the Arctic or Antarctica.
Concept Introduction:
Temperature is measure of the warmth or coldness of an object or substance.
Isotope are the variants of same element having same number of proton with different mass number. Examples
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students 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.)
Hw.60.
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 21 Solutions
Chemistry: Atoms First
Ch. 21.2 - The bond enthalpy of O2 is 49S.7 kJ/mol. Calculate...Ch. 21.2 - Prob. 1PPACh. 21.2 - Prob. 1PPBCh. 21.2 - Prob. 1PPCCh. 21.2 - Prob. 21.2.1SRCh. 21.2 - Prob. 21.2.2SRCh. 21.5 - Prob. 21.2WECh. 21.5 - Prob. 2PPACh. 21.5 - Prob. 2PPBCh. 21.5 - Prob. 2PPC
Ch. 21.5 - Prob. 21.5.1SRCh. 21.5 - Prob. 21.5.2SRCh. 21.8 - Prob. 21.3WECh. 21.8 - Prob. 3PPACh. 21.8 - Prob. 3PPBCh. 21.8 - Prob. 3PPCCh. 21.8 - Prob. 21.8.1SRCh. 21 - Prob. 21.1QPCh. 21 - Prob. 21.2QPCh. 21 - Prob. 21.3QPCh. 21 - Prob. 21.4QPCh. 21 - Prob. 21.5QPCh. 21 - Prob. 21.6QPCh. 21 - Prob. 21.7QPCh. 21 - Prob. 21.8QPCh. 21 - Prob. 21.9QPCh. 21 - Prob. 21.10QPCh. 21 - Prob. 21.11QPCh. 21 - Prob. 21.12QPCh. 21 - Prob. 21.13QPCh. 21 - Prob. 21.14QPCh. 21 - Prob. 21.15QPCh. 21 - Prob. 21.16QPCh. 21 - Prob. 21.17QPCh. 21 - Prob. 21.18QPCh. 21 - Prob. 21.19QPCh. 21 - Prob. 21.20QPCh. 21 - Prob. 21.21QPCh. 21 - Prob. 21.22QPCh. 21 - Prob. 21.23QPCh. 21 - Prob. 21.24QPCh. 21 - Prob. 21.25QPCh. 21 - Prob. 21.26QPCh. 21 - Prob. 21.27QPCh. 21 - Prob. 21.28QPCh. 21 - Prob. 21.29QPCh. 21 - Prob. 21.30QPCh. 21 - Prob. 21.31QPCh. 21 - Prob. 21.32QPCh. 21 - Prob. 21.33QPCh. 21 - Prob. 21.34QPCh. 21 - Prob. 21.35QPCh. 21 - Prob. 21.36QPCh. 21 - Prob. 21.37QPCh. 21 - Prob. 21.38QPCh. 21 - Prob. 21.39QPCh. 21 - Calcium oxide or quicklime (CaO) is used in...Ch. 21 - Prob. 21.41QPCh. 21 - Prob. 21.42QPCh. 21 - Prob. 21.43QPCh. 21 - Prob. 21.44QPCh. 21 - Prob. 21.45QPCh. 21 - Prob. 21.46QPCh. 21 - Prob. 21.47QPCh. 21 - Prob. 21.48QPCh. 21 - Prob. 21.49QPCh. 21 - Prob. 21.50QPCh. 21 - In which region of the atmosphere is ozone...Ch. 21 - The gas-phase decomposition of peroxyacetyl...Ch. 21 - Prob. 21.53QPCh. 21 - Prob. 21.54QPCh. 21 - Prob. 21.55QPCh. 21 - Prob. 21.56QPCh. 21 - Prob. 21.57QPCh. 21 - Prob. 21.58QPCh. 21 - A concentration of 8.00 102 ppm by volume of CO...Ch. 21 - Prob. 21.60QPCh. 21 - Briefly describe the harmful effects of the...Ch. 21 - Prob. 21.62QPCh. 21 - Prob. 21.63QPCh. 21 - Prob. 21.64QPCh. 21 - Prob. 21.65QPCh. 21 - Prob. 21.66QPCh. 21 - Prob. 21.67QPCh. 21 - A glass of water initially at pH 7.0 is exposed to...Ch. 21 - Prob. 21.69QPCh. 21 - Prob. 21.70QPCh. 21 - Describe the removal of SO2 by CaO (to form CaSO3)...Ch. 21 - Which of the following settings is the most...Ch. 21 - Prob. 21.73QPCh. 21 - Peroxyacetyl nitrate (PAN) undergoes thermal...Ch. 21 - Prob. 21.75QPCh. 21 - Prob. 21.76QPCh. 21 - The carbon dioxide level in the atmosphere today...Ch. 21 - A 14-m by 10-m by 3.0-m basement had a high radon...Ch. 21 - Prob. 21.79QPCh. 21 - A person was found dead of carbon monoxide...Ch. 21 - Prob. 21.81QPCh. 21 - As stated in the chapter, carbon monoxide has a...Ch. 21 - Prob. 21.83QPCh. 21 - Prob. 21.84QPCh. 21 - Prob. 21.85QPCh. 21 - Prob. 21.86QP
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
- What 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_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. Use dimensional analysisarrow_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
- For the reaction S(8) + O₂(g) → SO₂ (g) AH = -296 kJ per mole of SO₂2 formed. [Review Topics] a. Calculate the quantity of heat released when 1.78 g of sulfur is burned in oxygen. kj Submit Answer b. Calculate the quantity of heat released when 0.486 mol of sulfur is burned in air. kj c. What quantity of energy is required to break up 1 mole of SO2(g) into its constituent elements? kj Retry Entire Group [References] more group attempts remainingarrow_forwardBecause carbon and silicon are both elements in group 14 on the periodic table, we expect them to react with other elements in similar ways. To some extent, they do, but in some cases, carbon and silicon compounds that seem to have analogous structures have very different chemical characteristics. For example, carbon tetrachloride, CCl4, is very stable in the presence of water, but silicon tetrachloride, SiCl4, reacts quickly with water. The unbalanced equation for this reaction is SiCl4 + H2O → Si(OH)4 + HCl Balance this equation. Write a conversion factor that could be used to convert between moles of SiCl4 and moles of H2O. How many moles of SiCl4 react with 24 moles of water? Write a conversion factor that could be used to convert between moles of Si(OH)4 and moles of water. How many moles of Si(OH)4 form when 4.01 moles of H2O react with an excess of SiCl4?arrow_forwardThe 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_forward
- 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.arrow_forwardWe can use Hess's Law (and some creativity!) to learn about the energetics of reactions that occur in remote environments. Consider the atmospheric reaction, NO + O → NO₂ (a) Use the dissociation energy of O2, 498.34 kJ/mol, and the standard heats of formation for NO (+90.25 kJ/mol) and NO₂ (+33.18 kJ/mol) to derive the enthalpy change for this reaction. QUESTION 14 (b) The two bonds in NO2 are equivalent, and we can use the bond strength of N₂, 945 kJ/mol, and the information given in part (a) to determine ArxnH for N+O+O→ NO₂ From this ArxnH, estimate the bond strength of each of the resulting N-O bonds in kJ/mol. (Note: Your answer for this part does not necessarily depend on your answer to part a).arrow_forwardMuch of the U.S. electricity is generated in thermal generating stations that burn fossil fuels such as coal and natural gas. The use of solar-powered generating stations is expected to increase over the next decade and replace older fossil-fuel generating stations. What impact might this change have on greenhouse gas emissions?arrow_forward
- Which statement is correct?arrow_forwardHow many kg of CO2 are emitted from an automobile that completely combusts all the gasoline in its 13.9 gallon fuel tank? You may assume that gasoline is entirely octane, which has the following combustion equation: 2 C3H18 (1) + 25 O2 (g) → 16 CO2 (g) + 18 H20 (g) Useful information: 1 gallon = 3.7854 L. • This combustion occurs in excess O2. • The density of octane is p = 703 g/L. • The molar mass of CO, is 44.01 g/mol. • The molar mass of octane is 114.23 g/mol. Answer:arrow_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 32.2 × 104 kJ of heat?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
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
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 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
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
Types of Matter: Elements, Compounds and Mixtures; Author: Professor Dave Explains;https://www.youtube.com/watch?v=dggHWvFJ8Xs;License: Standard YouTube License, CC-BY