T (°C) 2.2 24.5 38.8 Average K .00061 .00075 .00084 Complete the following table and calculate the enthalpy, entropy, and Gibbs' energy of the reaction. Enter your answers in the questions below as indicated here: T(K) Cold Temp. Room Temp. Hot Temp. Slope Intercept AH° ASO AG (at 50 °C) 275.35 297.65 311.95 1/T (1/K) 0.0036 0.0034 0.0032 -4.63 -38.49 A) Find Slope in Units of K 13) Find AH c) Find AG at 50°C ? ? ? In(K) -7.4 7.2 -7.08 -

T (°C) 2.2 24.5 38.8 Average K .00061 .00075 .00084 Complete the following table and calculate the enthalpy, entropy, and Gibbs' energy of the reaction. Enter your answers in the questions below as indicated here: T(K) Cold Temp. Room Temp. Hot Temp. Slope Intercept AH° ASO AG (at 50 °C) 275.35 297.65 311.95 1/T (1/K) 0.0036 0.0034 0.0032 -4.63 -38.49 A) Find Slope in Units of K 13) Find AH c) Find AG at 50°C ? ? ? In(K) -7.4 7.2 -7.08 -

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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Use the data provided in the table to calculate the change in Gibbs Free-Energy at 25 degrees Celsius for the reaction given. Ag+ (aq) Cl- (aq) AgCl (s) S0 (J K-1 mole-1) 72.68 56.4 96.2 Delta H Kj/mol 105.58 -167.2 -127.07 Group of answer choices -75.2 kJ +55.7 kJ +32.5 kJ -75.2 kJ -55.7 kJ
The equilibrium constant for a system at chemical equilibrium at 318 oC is 3.4 x 10-3. Calculate the Gibbs free-energy change, deltaGo, for the system at 318 oC.Enter your answer here: kJ/mol
Σ *00 <(0 Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Refer to the AG°; values. Fe,0,(s) +2 Al(s)→ Al, O, (s) + 2 Fe(s) AG° rxn 8:12 PM 11/8/2021 PrtScr Delete Insert F11 F8 こレ F6 F7 F4 Backspace %24 % %23 80 C. Alt Ctrl Home
In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °C and constant total pressure. Then, she 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 her 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. P₂010 (s) + 6H₂0 (1) 4H₂ PO(s) 4 2NH₂ (g) → N₂H₂(g) + H₂ (g) 2 4 2 ΔΗ = -439. kJ AS-1179. AG = AH = k AS = kJ Which is spontaneous? this reaction the reverse reaction neither 188. kJ OK- K J K AG 16. kJ Which is spontaneous? this reaction the reverse…
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Estimate the temperature in K at which the reaction will become nonspontaneous.
Calculate E°cell in V for a reaction with K. = 6.99 x 10-15 and n = 4. Your Answer: Answer units
13. For the reaction, 250, (g) + 02 (g) 2- 250, (g), K. = 9 x 102 at 800 K, and K. = 1 x 10 at 635 K. Which of the following is wrong about this reaction? A) It is an exothermic reaction. B) At 800 K, SO, molecules are more stable than %3D %3D those at 635 K, C) The heat content of SO, molecules is less than that of SO, molecules. D) K, is smaller than Ke at 800 K. E) The rátio of specific rate constant for forward re- action to that of the reverse reaction at 635 K is 1x10.
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
The following reaction has these standard thermodynamie parameters: An-30.6 kmol and AS 55.3 J(mol K).
Calculate AG°for the combustion of propane. C3H8(g) + 502(g) → 3CO2(s) + 4H20(g) Standard Thermodynamic Properties for Selected Substances Substance AH; (kJ mol-) AG; (kJ mol-1) S° (JK-1 mo Co3 2 (aq) -677.1 -527.8 -56.9 CH4(g) -74.6 -50.5 186.3 CH3OH() -239.2 -166.6 126.8 CH3OH(g) -201.0 -162.3 239.9 CCI4() -128.2 -62.5 214.4 CCIA(9) -95.7 -58.2 309.7 CHCI3() -134.1 -73.7 201.7 CHCI3(g) -103.14 -70.34 295.71 CS2() 89.70 65.27 151.34 CS2(g) 116.9 66.8 238.0 209 2 200.9 027 4
Species AG° Fe(OH)3 -696.5 Fe+ -4.6 OH -157.3 Calculate the AG° of the reaction: Fe(OH)3(s) = Fe*(aq) + 3 OH (aq) T= 25° C Express the answer to 1 decimal place. kJ