4. From the AH acerate. in question 3, calculate the J/g and J/mol of the solid...
Question 19 of 21 > Attempt 3 Indicate the direction of polarity of each of the covalent bonds by placing the appropriate delta notation next to each end of the bond. Answer Bank o C- 0 0— 1 0—F C—N C1— S- H S-C1
Indicate the direction of polarity of each of the covalent bonds by placing the appropriate delta notation next to each end of the bond. 0- 0 Answer Bank 0401 C- N S— H S- C1
Indicate the direction of polarity of each of the covalent bonds by placing the appropriate delta notation next to e the bond. Answer Bank B0—F B —No s-H DB s—C1 o -
Indicate the direction of polarity of each of the following covalent bonds by dragging the appropriate delta notation to each end of the bond. C-O O-CL O-F C-N CL-C S-H S-CL
Using the values of Delta H and Delta S given, calculate Delta G for each of the reactions at 25 degree C and indicate whether the reactions are spontaneous or non-spontaneous. Explain. Delta H = 10.5 kJ/mol and Delta S = 30.0 J/K-mol Delta H = -10.5 kJ/mol and Delta S = 105. J/K-mol
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
4. Use the bond enthalpies below and calculate the enthalpy of ethane combustion in kJ / mol. (AH° (H-H) = 436 kJ mol', AH° (C-H) = 435 kJ mol', AH° (0=0) = 498, AH° (CEO) = 732, AH (H-O) = 463] CzH6 (g) + 7/202 (g) - 2002 + 3H20 (g)
11. Given the values for H (2.1) and Cl (3.0), calculate the electronegativity difference in a hydrogen chloride bond, HCl. 36) ______ A) -0.9 B) 0.9 C) 5.1 D) -5.1 E) none of the above 12 A sample of krypton gas at 75.0 psi expands from 0.100 L to 0.450 L. If the temperature remains constant, what is the final pressure in psi? 37) ______ A) 0.167 psi B) 16.7 psi C) 3.38 psi D) 75.0 psi E) 338 psi 13. Which of the following...
24. Calculate the change in AH kJ mol enthalpy (in J per mole of NaHCO (5) -947.7 CO) for the decomposition Na.co.(s) -1130.9 of sodium hydrogen H.00) -241.8 carbonate from CO.() -393.5 the standard enthalpies of formation 2 NaHCO3(5) - Na.CO() + H2009) + COUP) (A) 129.2 (B) -818.5 (C) -1766.2 (D) -3661.6
1. Calculate the bond energy of the CI-F bond using the following data: Cl2(g) + F2(g) → 2CIF(g) AH = -108 kJ Bond enthalpies (kJ/mol): CI-CI (239); F-F (159) CI-C1 = 239 F.F : 159 1 2. Find the experimental Lattice energy of aluminum oxide using a Born-Haber cycle using the following information: AH® (aluminum oxide) = -1676 kJ/mol IE, (aluminum) = 577.6 kJ/mol IE, (aluminum) =1816.7 kJ/mol IE(aluminum) = 2744.8 kJ/mol AH® (aluminum atom, g) = 329.7 kJ/mol AHⓇEAI...