Chemistry
13th Edition
ISBN: 9781259911156
Author: Raymond Chang Dr., Jason Overby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 22, Problem 22.52QP
From the data in Appendix 2, calculate ΔH° for the synthesis of NO (which is the first step in the manufacture of nitric acid) at 25°C:
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Chemistry
Ch. 22 - Prob. 22.1QPCh. 22 - Prob. 22.2QPCh. 22 - Prob. 22.3QPCh. 22 - Carbon is usually classified as a nonmetal....Ch. 22 - Prob. 22.5QPCh. 22 - Describe two laboratory and two industrial...Ch. 22 - Prob. 22.7QPCh. 22 - Prob. 22.8QPCh. 22 - Prob. 22.9QPCh. 22 - Describe what is meant by the hydrogen economy.
Ch. 22 - Elements number 17 and 20 form compounds with...Ch. 22 - Give an example of hydrogen as (a) an oxidizing...Ch. 22 - Prob. 22.13QPCh. 22 - Prob. 22.14QPCh. 22 - Prob. 22.15QPCh. 22 - Prob. 22.16QPCh. 22 - Prob. 22.17QPCh. 22 - Starting with H2, describe how you would prepare...Ch. 22 - Give an example of a carbide and a cyanide.Ch. 22 - How are cyanide ions used in metallurgy?Ch. 22 - Briefly discuss the preparation and properties of...Ch. 22 - Prob. 22.22QPCh. 22 - Prob. 22.23QPCh. 22 - Describe two chemical differences between CO and...Ch. 22 - Describe the reaction between CO2 and OH in terms...Ch. 22 - Prob. 22.26QPCh. 22 - Prob. 22.27QPCh. 22 - Prob. 22.28QPCh. 22 - Prob. 22.29QPCh. 22 - Magnesium chloride is dissolved in a solution...Ch. 22 - Prob. 22.31QPCh. 22 - Prob. 22.32QPCh. 22 - A piece of red-hot magnesium ribbon will continue...Ch. 22 - Prob. 22.34QPCh. 22 - Describe a laboratory and an industrial...Ch. 22 - Prob. 22.36QPCh. 22 - Prob. 22.37QPCh. 22 - Prob. 22.38QPCh. 22 - Prob. 22.39QPCh. 22 - Prob. 22.40QPCh. 22 - Prob. 22.41QPCh. 22 - Write a balanced equation for the formation of...Ch. 22 - Prob. 22.43QPCh. 22 - At 620 K the vapor density of ammonium chloride...Ch. 22 - Prob. 22.45QPCh. 22 - Prob. 22.46QPCh. 22 - Write a balanced equation for each of the...Ch. 22 - Prob. 22.48QPCh. 22 - Prob. 22.49QPCh. 22 - Predict the geometry of nitrous oxide, N2O, by the...Ch. 22 - Consider the reaction N2(g)+O2(g)2NO(g) Given that...Ch. 22 - From the data in Appendix 2, calculate H for the...Ch. 22 - Prob. 22.53QPCh. 22 - Prob. 22.54QPCh. 22 - Prob. 22.55QPCh. 22 - Prob. 22.56QPCh. 22 - Prob. 22.57QPCh. 22 - Prob. 22.58QPCh. 22 - Describe one industrial and one laboratory...Ch. 22 - Prob. 22.60QPCh. 22 - Prob. 22.61QPCh. 22 - Prob. 22.62QPCh. 22 - Describe the contact process for the production of...Ch. 22 - Prob. 22.64QPCh. 22 - Prob. 22.65QPCh. 22 - One of the steps involved in the depletion of...Ch. 22 - Hydrogen peroxide is unstable and decomposes...Ch. 22 - What are the oxidation numbers of O and F in HFO?Ch. 22 - Prob. 22.69QPCh. 22 - In 2008, about 48 million tons of sulfuric acid...Ch. 22 - Prob. 22.71QPCh. 22 - Prob. 22.72QPCh. 22 - Prob. 22.73QPCh. 22 - Prob. 22.74QPCh. 22 - Prob. 22.75QPCh. 22 - Prob. 22.76QPCh. 22 - Describe two reactions in which sulfuric acid acts...Ch. 22 - Prob. 22.78QPCh. 22 - Prob. 22.79QPCh. 22 - Prob. 22.80QPCh. 22 - Prob. 22.81QPCh. 22 - Prob. 22.82QPCh. 22 - Prob. 22.83QPCh. 22 - Prob. 22.84QPCh. 22 - Prob. 22.85QPCh. 22 - Hydrogen fluoride can be prepared by the action of...Ch. 22 - Prob. 22.87QPCh. 22 - Prob. 22.88QPCh. 22 - Use the VSEPR method to predict the geometries of...Ch. 22 - Iodine pentoxide, I2O5, is sometimes used to...Ch. 22 - Prob. 22.91QPCh. 22 - Prob. 22.92QPCh. 22 - Prob. 22.93QPCh. 22 - What is the change in oxidation number for the...Ch. 22 - Prob. 22.95QPCh. 22 - Prob. 22.96QPCh. 22 - Prob. 22.97QPCh. 22 - Consider the Frasch process. (a) How is it...Ch. 22 - Predict the physical and chemical properties of...Ch. 22 - Prob. 22.100QPCh. 22 - Prob. 22.101QPCh. 22 - Life evolves to adapt to its environment. In this...Ch. 22 - Prob. 22.103QPCh. 22 - As we saw in Section 21.2, the reduction of iron...Ch. 22 - Assuming ideal behavior, calculate the density of...Ch. 22 - A 10.0-g sample of white phosphorus was burned in...
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- Data are given in Appendix 1 for white phosphorus, P4(s). P4(g) has the following thermodynamic values: Hf=58.9kJ/mol , S=280.0J/kmol . What is the temperature at which white phosphorus sublimes at 1 atm pressure?arrow_forwardThe major industrial use of hydrogen is in the production of ammonia by the Haber process: 3H2(g)+N2(g)2NH3(g) a. Using data from Appendix 4, calculate H, S, and G for the Haber process reaction. b. Is the reaction spontaneous at standard conditions? c. At what temperatures is the reaction spontaneous at standard conditions? Assume H and S do not depend on temperature.arrow_forwardUse the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.arrow_forward
- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardFrom the data given in Appendix I, determine the standard enthalpy change and the standard free energy change for each of the following reactions: (a) BF3(g)+3H2O(l)B(OH)3(s)+3HF(g) (b) BCl3(g)+3H2O(l)B(OH)3+3HCl(g) (c) B2H6(g)+6H2O(l)2B(OH)3(s)+6H2(g)arrow_forwardCalcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?arrow_forward
- Use the standard free energy of formation data in Appendix G to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 C. Identify each as either spontaneous or nonspontaneous at these conditions. (a) MnO2(s)Mn(s)+O2(g) (b) H2(g)+Br2(l)2HBr(g) (c) Cu(s)+S(g)CuS(s) (d) 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(g) (e) CH4(g)+O2(g)C(s,graphite)+2H2O(g) (f) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)arrow_forwardCalcium 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_forwardUsing data from Appendix 4, calculate H, S and G for the following reactions that produce acetic acid: Which reaction would you choose as a commercial method for producing acetic acid (CH3CO2H) at standard conditions? What temperature conditions would you choose for the reaction? Assume H and S do not depend on temperature.arrow_forward
- Use data from Appendix J to calculate the enthalpy change and the Gibbs free energy change for the reduction of chromium(III) oxide by aluminum.arrow_forwardConsider the Haber process: N2(g)+3H2(g)2NH3(g);H=91.8kJ The density of ammonia at 25C and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol C). (a) How much heat is evolved in the production of 1.00 L of ammonia at 25C and 1.00 atm? (b) What percentage of this heat is required to heat the nitrogen required for this reaction (0.500 L) from 25C to 400C, the temperature at which the Haber process is run?arrow_forwardUsing data from Appendix 4, calculate G for the reaction 2H2S(g)+SO2(g)3Srhombic(s)+2H2O(g) for the following conditions at 25C: PH2S=1.0104atmPSO2=1.0102atmPH2O=3.0102atmarrow_forward
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