Given the following thermodynamic data calculate ΔS and ΔSsurr for the following reaction at 25°C and...
Given the following unbalanced reaction and thermodynamic information, what is AGºrxn at 35 °C? Please report your answer to the correct number of significant figures and pay attention to the units to which you are asked to report your answer to. C5H12 (1) + O2 (g) → CO2 (g) + H20 (g) AHºf values (kJ/mol): C5H12 (1) = -174; CO2 (g) = -394; H20 (g) = -242 Sº values (J/Kmol): C5H12 (1) = 317 ; CO2 (g) = 214; H20...
Use the given data at 700 K to calculate ΔG°for the reaction H2(g) + CO2(g) → H2O(g) + CO(g) Substance H2(g) CO2(g) H2O(g) CO(g) ΔH°f(kJ/mol) 0 -393 -242 -111 S°(J/K·mol) 131 214 189 198 -472 kJ 10.6 kJ -775 kJ -2.94 x 104 kJ
solve questions 18 and 19 please How anch work can be done using a 1.50-V alkaline battery in which 2 moles of electrons are transferred tioni the anode to the cathode? IS. 19. Because of recent advances in recovery technology, the supply of natural gas. which is mostly methane. has increased signiticanrly. It I mole of methane is cousumed in a fuel cell powering an automobile. estimate d) how much work is produced. and 2) the voltage produced by the...
MAIN QUESTIO Given the following thermodynamic data calculate AS for the following reaction at 25°C and 1 atm: XeF(9) —— XeFe(s) + Fz(9) AH®: (kJ/mol) S (J/K-mol) XeF6(9) -294 300. XeF(s) -251 146 F2(g) 10 203
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) CO2(g) 214 H2O(l) 189 CH4(g) 186 O2(g) 205
For the following reaction: 2 CO(g) + O2(g) → 2 CO2(g), given ΔH = -566 kJ and ΔG = -514 kJ, find ΔS (J/K) at 25 oC. Multiple Choices: ΔS = -174 J/K ΔS = -0.174 J/K ΔS = -2.08J/K ΔS = 174 J/K ΔS = -2080 J/K
Use the given data at 500 K to calculate ΔG°for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance H2S(g) O2(g) H2O(g) SO2(g) ΔH°f(kJ/mol) -21 0 -242 -296.8 S°(J/K·mol) 206 205 189 248
Consider the reaction listed below along with the accompanying thermodynamic data, carried out at 25 °C and 1 atm: 2SO2(g) + O2(g) ↔ 2SO3(g) Substance ∆Hf° (kJ/mol) S° (J/K • mol) SO2(g) -297 248 O2(g) 0 205 SO3(g) -396 257 A.Calculate ∆H°. B. Calculate ∆S°. C. Calculate ∆G°. Is this reaction spontaneous? Briefly explain. D. At what temperature will this reaction first become spontaneous? E. Calculate the equilibrium constant for this reaction.
Use the table below to answer question 1. Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AHºf (kJ/mol) AG°f (kJ/mol) S (J/K-mol) 2.84 2.43 Sige Carbon C(s, diamond) 1.88 C(s, graphite) 0 C2H2 (g) 226.7 C2H4 (g) 52.30 C2H6 (g) -84.68 CO(g) -110.5 CO2 (g) -393.5 209.2 68.11 -32.89 -137.2 -394.4 5.69 200.8 219.4 229.5 197.9 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2 (g) H20 (1) 205.0 69.91 -285.83 -237.13 1) The combustion of acetylene in...