∑ m∆H°f (products) - ∑n∆H°f (reactants), where m and n are coefficients.
Substance --- ΔH° (kJ mol–) --- ΔG° (kJ
mol–1) --- S°298 (J K–1
mol–1)
C2H4 52.4 86.4 219.3
H2 0 0 130.7
C2H6 -84.0 -32.0 229.2
CO -110.52 -137.15 197.7
H2O -285.83 -237.1 70.0
CO2 -393.51 -394.36 213.8
NO2 33.2 51.30 240.1
NO 90.25 87.6 210.8
SO2 -296.83 -300.1 248.2
O2 0 0 205.2
SO3 -395.72 -371.06 256.76
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ...
Use data from the table below to calculate the equilibrium constants at 25∘C for each reaction. Standard Thermodynamic Quantities for Selected Substances at 25∘C Substance ΔH∘f(kJ/mol) ΔG∘f(kJ/mol) S∘(J/mol⋅K) H2(g) 0 0 130.7 N2(g) 0 0 191.6 O2(g) 0 0 205.2 NO(g) 91.3 87.6 210.8 NO2(g) 33.2 51.3 240.1 CO(g) -110.5 -137.2 197.7 CO2(g) -393.5 -394.4 213.8 H2S(g) -20.6 -33.4 205.8 S2(g) 128.6 79.7 228.2 1. N2(g)+O2(g)⇌2NO(g)
Use data given below to calculate ΔrS∘ΔrS∘ for each of the reactions. Standard Thermodynamic Quantities for Selected Substances at 25 ∘C∘C Substance ΔrS∘ΔrS∘, JK−1mol−1JK−1mol−1 Cr(s)Cr(s) 23.8 Cr2O3Cr2O3(s)(s) 81.2 CO(g)CO(g) 197.7 CO2(g)CO2(g) 213.8 H2(g)H2(g) 130.7 H2O(g)H2O(g) 188.8 H2O(l)H2O(l) 70.0 HNO3(aq)HNO3(aq) 146.0 N2(g)N2(g) 191.6 N2O4(g)N2O4(g) 304.4 NO(g)NO(g) 210.8 NO2(g)NO2(g) 240.1 O2(g)O2(g) 205.2 SO2(g)SO2(g) 248.2 SO3(g)SO3(g) 256.8 A) 4NO2(g)+2H2O(l)+O2(g)→4HNO3(aq) B) Cr2O3Cr2O3(s)(s) +3CO(g)→2Cr(s)+3CO2(g) C) SO2(g)SO2(g) +12O2(g)→SO3(g) D) N2O4(g)+4H2(g)→N2(g)+4H2O(g)
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) + H2(g) + C2H6(g) ΔΗ° Substance (kJ/mol) C₂H4 52.4 C2H6 -84.68 0 -32.3 kJ -4.3 x 103 kJ 32.3 kJ 0 -137.1 kJ
C2H4(g)+H2(g)→C2H6(g) Exercise 18.55 24 of 37 > MI Review | Constants Periodic Table Use data from the table below to calculate AS each of the following reactions. for Part A S" (J/mol. K) 197.7 213.8 130.7 CH,(g) + H, (g) → C, H. (g) Express your answer using one decimal place. 188.8 EVO AXO AO ? Substance CO(9) CO,(9) H,(9) H.O(9) 0 (9) C,H. (9) C, H. (9) C(s) SO (9) so (9) CH, OH(g) ASIL J/K 205.2 219.3 229...
Calculate the entropy of the following reaction, using the table below. Enter your answer without units to one decimal. 2C6H6(g) + 15O2 (g) → 12CO2 (g) + 6H2O (g) Substance ΔHf° (kJ/mol) ΔGf° (kJ/mol) S° (J/mol∙K) CH3COOH (g) -484.3 -389.9 159.8 (CH3)2O (g) -184.1 -112.6 266.4 C2H6 (g) -84.0 -32.0 229.2 C2H5OH (g) -234.8 -167.9 281.6 C6H6 (g) 82.9 129.7 269.2 CO2 (g) -393.5 -394.4 213.8 H2O (g) -241.8 -228.6 188.8 H2O (l) -285.8 -237.1 70 O2 (g) 0.0 0.0...
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)
Use the Data table to calculate ∆H for the reaction below:Reactions: Change in Enthalpy (∆H)(1) C (s) + O2 (g) -> CO2(g) ∆H1 = -393.5 kJ/ mol(2) H2 (g) + 1/2 O2 (g) -> H2O (l) ∆H2 = -285.8 kJ/mol(3) 2C2H6 (g) + 7O2 (g) -> 4 CO2 (g) + 6 H2O (l) ∆H3 = -283.0 kJ/molCalculate the enthalpy change for the reaction:2 C (s) + 3 H2 (g) -> C2H6(g) ∆H = ______________kJ/mol
Practice with Hess's Law and Standard Heats of Formation 1. (Example) The reaction C2H4 (g) + 6 F2 (g) → 2 CF4(g) + 4 HF (g) can be written as the sum of: C2H4 (9) ► 2 C(s) + 2 H2 (g) AH = -52.3 kJ/mol 2 C(s) + 4 F2 (9) ► 2 CF4(9) AH = -1360 kJ/mol 2 H2(g) + 2 F2 (g) → 4 HF (a) AH = -1074 kJ/mol C2H4(g) + 6 F2(g) → 2 CF4(g)...
2. Given the following heats of formation, calculate AH for the reaction 2 CO(g) + 5 H2(g) → C2H6 (g) + 2 H2O(g) Compound AH°F (kJ/mol) Compound AH°F (kJ/mol) 52.28 C₂H6 (8) -84.68 C2H4 (8) -393.5 CO2(g) -241.8 H2O(g) -285.9 CO(g) -110.5 H2O(1)
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(l) For C6H12(l), ΔH°f = –151.9 kJ/mol (5 points) Substance ∆H°f , kJ/mol C6H12(l) –151.9 O2(g) 0 H2O(l) –285.8 CO2(g) –393.5 2).Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according to the equation N2(g) + 3H2(g) → 2NH3(g) ΔH°= –92.6 kJ/mol Assume that the reaction takes place under standard conditions at 25oC.