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- Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.The enthalpy of sublimation of calcium at 25 °c is 178.2 kJ mol- 1.How much energy (at constant temperature and pressure) must be supplied as heat to 5.0 g of solid calcium to produce a plasma (a gas of charged particles) composed of Ca2+ ions and electrons?
- MISSED THIS? Read Section 19.8 (Pages 871-877); Watch IWE 19.6. Liquid methanol burns in oxygen to form gaseous carbon dioxide and gaseous water. Substance H (kJ/mol) S° (J/(mol · K)) CH, OH (1) -238.6 126.8 O₂(g) 0 205.2 CO₂(g) -393.5 213.8 CO2(aq) -413.8 117.6 H₂O(g) -241.8 188.8 H₂O(1) -187.8 70.0 ▼ Part D where no represents the stoichiometric coefficients of the products, n, represents the st of the reactants, and Sº represents the standard entropies. AGxn= Calculate AG at 25°C. Express your answer in kilojoules to three significant figures. Submit = Provide Feedback 15] ΑΣΦ Request Answer Part E Complete previous part(s) [2(S° co₂(g)) + 4(S° H₂O(g))]- [2(S° CH₂OH()) + 3(S° 0₂(E [2(213.8 J/K)+4(188.8 J/K)] - [2(126.8 J/K) + 3(2 314 J/K MacBook Pro P Pearson ? kJ Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions ContacThe term "bond energy" and "bond enthalpy" have often been used interchangeably to describe the strength of a bond. a) Calculate the average bond enthalpy of the O-H bond in water at 298 K and 1 bar, given the reaction: H₂O(g) →2H(g) + O(g), with AHƒ = 218.0, 249.2, and -241.8 kJ mol¹¹ for H(g), O(g), and H₂O(g) respectively. Give your answer in units of kJ/mol. b) How does your answer from (a) compare to the average bond energy (i.e. AU) of the O-H bond at 298 K and 1 bar: 461.0 kJ/mol?Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes iron to corrode in air is given by 4Fe +302-2Fe2O3 in which at 298 K, AH = - 1684 kJ and ASixn - 543.7 J/K. = Part C At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units. ► View Available Hint(s) Teq = Submit 14 μÅ Value Units ?
- The hydrocarbons acetylene (C2H2) and benzene (C6H6)have the same empirical formula. Benzene is an “aromatic”hydrocarbon, one that is unusually stable because of its structure.(a) By using data in Appendix C, determine the standardenthalpy change for the reaction 3 C2H2(g)-----> C6H6(l).(b) Which has greater enthalpy, 3 mol of acetylene gas or1 mol of liquid benzene? (c) Determine the fuel value, inkJ/g, for acetylene and benzene.What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ► View Available Hint(s) Submit AGixn = 6.24. 10¹¹ Part B AGrxn= xa Submit Part C μÅ Xb b Teq = Previous Answers X Incorrect; Try Again; 5 attempts remaining Enter your answer with a different unit type. Review a list of acceptable units. What is the Gibbs free energy for this reaction at 5975 K ? Assume that AH and AS do not change with temperature. Express your answer to two decimal places and include the appropriate units. ► View Available Hint(s) Value μА Value . μA X.10n J K X Units At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units. ► View Available Hint(s) Units ? ?(b) (i) Mixtures of molten salts often result in high excess mixing enthalpies. Calorimetric experiments of a 25:75 mixture of NaCl and KCl revealed an enthalpy of mixing ΔmixH of -0.4095 kJ mol-1 . Calculate β for this mixture. (ii) Aluminium boils at 2737 K at 100.0 kPa pressure. Given that at 100.0 kPa the molar heat capacity (Cp) of liquid aluminium is 29.30 J K-1 mol-1 , and of aluminium gas is 20.79 J K-1 mol-1 , calculate the total entropy change for the reaction: Al(liquid, 2000 K) → Al (gas, 3500 K). ΔvapS = 49.24 J K-1 mol-1
- Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T' is temperature, and S is entropy. The chemical reaction that causes aluminum to corrode in air is given by 4A1+30₂-2Al₂O₁ in which at 298 K, AH = -3352 kJ and AS = -625.1J/K Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K Express your answer as an integer and include the appropriate units. ▸ View Available Hint(s) μA AG - 89 kJ Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining Part B What is the Gibbs free energy for this reaction at 5975 K? Assume that AH and AS do not change with temperature. Express your answer to two decimal places and include the appropriate units. > View Available Hint(s) ? AG= Value Units SubmitThe diagram shows four states of a system, each with differentinternal energy, E. (a) Which of the states of the systemhas the greatest internal energy? (b) In terms of the ΔEvalues, write two expressions for the difference in internalenergy between State A and State B. (c) Write an expressionfor the difference in energy between State C and State D.(d) Suppose there is another state of the system, State E,and its energy relative to State A is ΔE = ΔE1 + ΔE4. Wherewould State E be on the diagram?How much energy (at constant temperature and pressure) must be supplied as heat to 10.0 g of chlorine gas (as Cl2) to produce a plasma composed of Cl- and Cl+ ions? The enthalpy of ionization of Cl(g) is +12575 kJ mol-1 and its electron gain enthalpy is -349 kJ mol-1. Hence identify the standardenthalpy of ionization of Cl- (g).