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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EBK 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
- Write a balanced equation for the formation of CO2(g) from C(s) and O2(g). Calculate the enthalpy change for this reaction using the following data (at 25 degrees Celsius): C(s) + 1/2 O2(g) --> CO(g) change in H = -111 kJ CO(g) + 1/2 O2(g) --> CO2(g) change in H = -394 kJ Is the reaction endothermic or exothermic?arrow_forwardConsider the two products CO2 and H2O for the combustion of ethanol. Use what you have learned about molecular geometry, polarity, and intermolecular forces to explain why CO2 is a gas at room temperature but H2O is a liquid at room temperature.arrow_forwardThe enthalpy of formation of CF4(g) is -679.9 kJ/mol. Based on the enthalpy of formation of two reactions, which is more exothermic? (See attached image)arrow_forward
- Are these reactions possible?arrow_forwardGiven the following heat of formation values, calculate the heat of reaction for the following: C3H8(g) + O2(g) → CO2(g) + H2O(l). ΔHf value in kJ/mol for C3H8(g) is −103.8, for O2(g) is 0, for CO2(g) is −393.5, and for H2O(l) is −285.8. 3.613 × 102 kJ 1.413 × 102 kJ −2.220 × 103 kJ −5.755 × 102 kJarrow_forward4. Write the balanced formation reaction, including physical states, for liquid tribromomethane, CHBr3.arrow_forward
- Consider the following reaction: 4 FeS2 (s) + 11 O2 (g) ↔ 2 Fe2O3 (s) + 8 SO2 (g) What is true about this process? A. ΔH > 0 and the reactants are energetically favored B. ΔH < 0 and the reactants are energetically favored C. ΔH < 0 and the products are energetically favored D. ΔH > 0 and the products are energetically favoredarrow_forwardGiven the following at 25°C and 1.00 atm: 1/2 N2(g) + O2(g) → NO2(g) ΔH° +33.2 kJ N2(g) + 2 O2(g) → N2O4(g) ΔH° +11.1 kJ Calculate the ΔH° for the reaction below at 25°C. 2 NO2(g) → N2O4(g)arrow_forwardIn the following molecular reaction, carbon is reduced. Explain how. In your explanation, also discuss oxygen’s effect on carbon’s electron density as a reactant and as a product. CO2(g) + H2(g) → CO(g) + H2O(g)arrow_forward
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