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Concept explainers
Interpretation: The Lewis electron dot structures for
Concept introduction:
Lewis dot structure: For a given molecule, the bonding concerning the atoms and also the lone pairs can be shown by the diagram.
In this structure a single bond is represented by one dot pair and double bond is represented by two dot pairs and so on.
VSEPR Theory [Valence Shell Electron Pair Repulsion Theory]:
Geometry of the molecules can be predicted using VSEPR Theory. It is based on the number of electron pairs around the central atom of the molecule. Depending upon the bond pairs and lone pairs, geometries can be classified as linear, bent, pyramidal, trigonal planar, tetrahedral, octahedral and so on.
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Chapter 20 Solutions
Chemistry & Chemical Reactivity
- 4a Assume that worldwide combustion of fossil fuel accounts for an energy use of 500 x 1015 kJ/year. Also, assume that all fossil fuels can be represented by the formula C3H5 with energy content of 32,500 kJ/kg.Finally, assume that air is 79% N2 and 21% O2 , and has a molecular weight of 29 kg/kmol. i. Estimate the annual release of CO2 to the atmosphere by burning fossil fuels, in kg/yr ii. If all that CO2 entered the atmosphere (and none was removed), estimate the increase in atmospheric concentration, in ppm by volume. Assume the atmosphere contains 6.7 x 1018 kg of air.arrow_forwardPlease help! Thank you!arrow_forwardUsing a table of average bond enthalpies. Table 6.2 ( Sec. 6-6b), estimate the enthalpy change for the industrial synthesis of methanol by the catalyzed reaction of carbon monoxide with hydrogen.arrow_forward
- 19 Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane using average bond enthalpies (use exam data sheet values). H–C≡C–H(g) + 2H2(g) → H3C–CH3(g)arrow_forward1. Ethene can react with steam to produce ethanol. (a) Write an equation for the reaction above. (b) i. Suggest a reason why the enthalpy change for the reaction cannot be measured directly. ii. Standard enthalpy of formation data can be used to calculate the enthalpy change of the reaction. Using the data from the table below, calculate the standard enthalpy change of the reaction. Molecule C₂H4 (8) H₂O(g) C₂H5OH (1) AH; (kJ mol-¹) +52.5 -241.8 -277.7 (c) Another way of producing ethanol is by reacting a chloroethane with aqueous sodium hydroxide. i. Name the type of reaction mechanism. ii. Explain what the words in your answer for part c(i) mean. iii. Draw the reaction mechanism for this reaction.arrow_forwardThe chemical equation for photosynthesis is as follows: 6 CO2 + 6 H2O → CoH1206 ( + 6 02 Every year, the mass of carbon dioxide used by this reaction on a small island is 2.85 x 10 kg. What is the annual enthalpy change resulting from photosynthesis on the island? Compound AH° (kJ/mol) -1268 02 CO2 -393.5 HO -285.8 O 303 x 10 k Q 2.54 x 10 k O 254 x 10 k O 153x 10' k 0412x 10 karrow_forward
- 1. 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_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_forwardHow does the heat produced when 1 mole ofC is burned directly to CO2by the reactionC(s) + O2(g)→CO2(g)compare with that produced when 1 mole ofC undergoes the two-step process:C(s) +12O2(g)→CO(g) morrison (gjm2355) – Chapter 17 – andrews – (7)2CO(g) +12O2(g)→CO2(g)if all reactants and products are at the same temperature and pressure? 1.The heat produced is the same either way. 2.More heat is produced in the two-step process. 3.Cannot tell without calculating the heat produced. 4.More heat is produced in the one-step process.arrow_forward
- What is the energy of one mole of photons having a wavelength of 550 nm and also find 2.045 g of a new compound with formula C9H8O2 is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 21.811 °C to 29.551 °C. [During calibration, the heat capacity of the calorimeter was found to be 11.75 kJ·°C-1.] What is ΔUcomb for this compound in kJ/mol?arrow_forwardWhat is the greenhouse effect? What are the potential long-term consequences of the greenhouse effect? How can we combat this problem?arrow_forwardWhat is the standard enthalpy of isomerization (kJ/mol) of propanol to isopropanol in the liquid state?arrow_forward
- Chemistry & 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 LearningEBK A SMALL SCALE APPROACH TO ORGANIC LChemistryISBN:9781305446021Author:LampmanPublisher:CENGAGE LEARNING - CONSIGNMENT
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
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