Enter your answer in the provided box. 0 Calculate AG for the following reaction at 25°C. You will have to look up the thermodynamic data. 2 C2H6g)+7 02(g)4 CO2(g)+6 H2O() kJ So (JIK mol) AG'f (kJ/mol) AHf (kJ/mol) Formula 229.5 -32.89 -84.7 C2H6 219.5 68.1 52.3 CНа CO(G) 197.9 -137.3 -110.5 CO2(9) 213.6 -394.4 -393.5 CO2(aq) 121.3 -386.2 -412.9 CO32- (aq) -53.1 -528.1 -676.3 HCO3 (aq) -587.1 94.98 -691.1 HаСОз(аg) 187.4 -699.7 -623.2 69.9 HаО() -285.8 -237.2 H2O(g) 188.7 -241.8 -228.6 197.9 COG) -137.3 -110.5 213.6 CO2(g) -394.4 -393.5 121.3 CO2(aq) O2(g) -386.2 -412.9 205.0 0 0 O3(aq) 16.3 -12.09 110.88 O3(g) 163.4 142.2 237.6 e ere to search F1 F2 F3 F4 F5 F6 F7 F8 F9 #

Enter your answer in the provided box. 0 Calculate AG for the following reaction at 25°C. You will have to look up the thermodynamic data. 2 C2H6g)+7 02(g)4 CO2(g)+6 H2O() kJ So (JIK mol) AG'f (kJ/mol) AHf (kJ/mol) Formula 229.5 -32.89 -84.7 C2H6 219.5 68.1 52.3 CНа CO(G) 197.9 -137.3 -110.5 CO2(9) 213.6 -394.4 -393.5 CO2(aq) 121.3 -386.2 -412.9 CO32- (aq) -53.1 -528.1 -676.3 HCO3 (aq) -587.1 94.98 -691.1 HаСОз(аg) 187.4 -699.7 -623.2 69.9 HаО() -285.8 -237.2 H2O(g) 188.7 -241.8 -228.6 197.9 COG) -137.3 -110.5 213.6 CO2(g) -394.4 -393.5 121.3 CO2(aq) O2(g) -386.2 -412.9 205.0 0 0 O3(aq) 16.3 -12.09 110.88 O3(g) 163.4 142.2 237.6 e ere to search F1 F2 F3 F4 F5 F6 F7 F8 F9 #

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the enthalpy change using the net ionic equation for the given neutralization reaction at 25 °C. The values of AH; can be found in the Thermodynamic Properties at 298 K table. BaBr₂(aq) + 2H₂O(1) Ba(OH)₂ (aq) + 2 HBr(aq) - - AH: neutralization 57.11 Incorrect kJ
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 105.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
What is the entropy change for the universe, DeltaSuniv (in J/K), when the reaction give below occurs at 425 K? 2 N2O (g) --> 2 N2 (g) + 2 O2 (g) DeltaHorxn= -165 kJ Som[N2O(g)] = +219 J/mole x K Som[N2 (g)] = +192 J/mole x K Som[O2 (g)] = +205 J/mole x K
The standard reaction free energy AG°= = -910. kJ for this reaction: 6C(a)+ 6H2(g)+ 3O2(g)->C6H12O(s) Use this information to complete the table below. Round each of your answers to the nearest kJ.
1. Using Hess's Law, calculate AH for this reaction: (T: 4) 2H3BO3(aq) →→→ B₂O3(s) + 3H₂O(l) (1) H₂BO3(aq) → HBO₂(aq) + H₂O(E) AH = -0.020 kJ (2) 2B₂O3(s) + H₂O(l) → H₂B4O7(s) AH = -17.5 kJ (3) H₂B4O7(s) + H₂O(l) → 4HBO₂(aq) AH = -11.3 kJ
Calculate AG° for the following reaction at 25°C. You will have to look up the thermodynamic data. 2 C,H6(g) + 7 02g) → 4 CO2(g) + 6 H20(1) kJ Formula AH (kJ/mol) AGʻ¡ (kJ/mol) S° (J/K - mol) C2H6 -84.7 -32.89 229.5 C2H4 52.3 68.1 219.5 Co(g) -110.5 -137.3 197.9 CO2(g) -393.5 -394.4 213.6 -386.2 121.3 CO2(aq) co,2-(aq) -412.9 -676.3 -528.1 -53.1 HCO3 (aq) -691.1 -587.1 94.98 H2CO3(aq) -699.7 -623.2 187 4 H20() -285.8 -237.2 69.9 H20(g) -241.8 -228.6 188.7 -137.3 197.9 Co(g) -110.5 -393.5 -394.4 213.6 CO2(9) CO2(aq) -412.9 -386.2 121.3 205.0 O2(g) Og(aq) -12.09 16.3 110.88 O3(g) 142.2 163.4 237.6
please help! use correct sig figs and/or scientific notation! Multiple part question and very confused. Also, at the end what would be the equilibrium constant for this reaction at 2500 ºC.
3. If 20 g of KNO3 is dissolved in 50 mL of water at 4 °C, is the system in equilibrium? If not, what spontaneous process will occur? What is the value of AG (NOT AG) for the system, as prepared, before any reaction occurs? KNO3, K², NO₂ (44) NO3(aq) AH R
This reaction is _______ (product or reactant) favored under standard conditions at 258 K
Determine the value of AG for the reaction at 309 K. Assume standard concentration 2NH;(g) = N,H,(g) + H, (g) Given AH (kJ/mol) S°J/{mol · K)) Substance NH3(3) -46.1 192.5 95.35 N2H4(g) H2(3) 238.5 0.0 130.6 O-87.0 kJ -182.5 kJ O -192.6 kJ O 87.0 kJ O 192.6 kJ
Please answer this with work shown! Thanks!