Concept explainers
(a)
Interpretation: The
Concept introduction: The
(b)
Interpretation: The
Concept introduction: The chemical reactions in which energy is released during the formation of products known as exothermic reactions. The energy released during the reaction is denoted by
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ORGANIC CHEMISTRY
- What is the likelihood that hydrogen (H2) will become a widely used fuel and that the hydrogen economy will become a reality? In particular, what are the advantages and disadvantages of H2 as a fuel? What would be necessary for a significant conversion to a hydrogen economy?arrow_forwardComparing the chemistry of carbon and silicon. (a) Write balanced chemical equations for the reactions of H2O() with CH4 (forming CO2 and H2) and SiH4 (forming SiO2 and H2). (b) Using thermodynamic data, calculate the standard free energy change for the reactions in (a). Is either reaction product-favored at equilibrium? (c) Look up the electronegativities of carbon, silicon, and hydrogen. What conclusion can you draw concerning the polarity of CH and SiH bonds? (d) Carbon and silicon compounds with the formulas (CH3)2CO (acetone) and [(CH3)2SiO]n (a silicone polymer) also have quite different structures. Draw Lewis structures for these species. This difference, along with the difference between structures of CO2 and SiO2, suggests a general observation about silicon compounds. Based on that observation, do you expect that a silicon compound with a structure similar to ethene (C2H4) exists?arrow_forwardFrom data in Appendix 4, calculate H, S, and G for each of the following reactions at 25C. a. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) b. 6CO2(g)+6H2O(l)C6H12O6(s)Glucose+6O2(g) c. P4O10(s) + 6H2O(l) 4H3PO4(s) d. HCl(g) + NH3(g) NH4Cl(s)arrow_forward
- What is a driving force? Name two common and important driving forces, and give an example of each. What is entropy? Although the total energy of the universe is constant, is the entropy of the universe constant? What is a spontaneous process?arrow_forwardConsider the following reaction:2CH3OH(g)→2 CH4(g) + O2(g) H=+252.8 kJ a. Is this reaction exothermic or endothermic? Explain briefly. b. Calculate the amount of heat transferred when 24.0 g of CH3OH(g) is decomposed by this reaction at constant pressure c. For a given sample of CH3OH, the enthalpy change during the reaction is 82.1 kJ. How many grams of methane, CH4, are produced? d. How many kilojoules of heat are released when 38.5 g of CH4 (g) reacts completely with O2 (g) to form CH3OH( g) at constant pressure?arrow_forwardCH,(9) + 2 O,(g) AH = -809.0 kJ/mol rxn Co,(9) + 2 H,0(g) ΔΗ. = -81.3 kJ 'cond 2 H,0U) Given the energy diagram above, what is AH when two moles of methane are combusted? -401.15 kJ +1604.6 kJ -802.3 kJ +802.3 kJ +401.15 kJ O -1604.6 kJarrow_forward
- A sample of a hydrocarbon is completely combusted in presence in O2(g) to produce 21.83 g carbon dioxide, 4.47 g H2O, and 311 KJ of heat. What is the mass of hydrocarbon sample that was combusted? What is the empirical formula of the hydrocarbon? Calculate the value of Ho per empirical-formula unit of the hydrocarbon. Do you think that the hydrocarbon is one of those listed in appendix C? Explain your answer.arrow_forwardCalculate ΔHo for each oxidation reaction. Attached equation is balanced as written; remember to take into account the coefficients in determining the number of bonds broken or formed. [ΔHo for O2 = 497 kJ/mol; ΔHo for one C=O in CO2 = 535 kJ/mol]arrow_forward
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