Determine if the photosynthesis reaction is spontaneous at 80°C.Chemical Equation: CO2 + H20 → C6H1206 + 02CompoundCO2H20C6H120602AS° (J/K•mol)213.669.9AH° (kJ/mol)-393.5-285.8-1274.5212.12051. Compute for the AH° rxn (kJ/mol) of the equation:(round off final answer to 1 decimal place)

Answered: Image /qna-images/answer/f5e533e1-f063-4951-8808-69d9e816f100.jpg

Determine if the photosynthesis reaction is spontaneous at 80°C. Chemical Equation: CO2 + H20 → C6H1206 + O2 AH° (kJ/mol) AS° (J/K•mol) 213.6 Compound CO2 H20 C6H1206 02 -393.5 -285.8 69.9 -1274.5 212.1 205 1. Compute for the AH° rxn (kJ/mol) of the equation: (round off final answer to 1 decimal place)

Determine if the photosynthesis reaction is spontaneous at 80°C. Chemical Equation: CO2 + H20 → C6H1206 + O2 AH° (kJ/mol) AS° (J/K•mol) 213.6 Compound CO2 H20 C6H1206 02 -393.5 -285.8 69.9 -1274.5 212.1 205 1. Compute for the AH° rxn (kJ/mol) of the equation: (round off final answer to 1 decimal place)

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...

See similar textbooks

Similar questions

8e. Consider the following reaction: Caco3 (s) → Cao (s) + CO2 (g) Data: A,H = +177.5 kJ mol1 A,S = +160.7 J mol1K1 At which temperature will the reaction become spontaneous?
Is this reaction spontaneous? Why or Why not? CaC2(s) + 2H2O(l) ---> C2H2(g) + Ca(OH)2(s) Delta H(rxn)= -128.9kJ Substances: CaC2(s)= S(1/mol*K)= 70.0 Delta H(f) (kJ/mol)= -59.8 H20(l)= S= 69.9 Delta H= -285.8 C2H2(g)= S= 200.8 Delta H= ? Ca(OH)2= S= 83.4 Delta H= -986.1
H+(aq) + OH-(aq) - - -> H2O (l) Use the table below to determine net ∆H for this reaction.
Calculate the standard entropy of formation of liquid ethanol at 25°C. [S0(Cgraphite) = 160.70J/K•mol, S0(O2) = 205.14 J/K•mol, S0(H2) = 130.68 J/K•mol, S0(C2H5OH) = 130.68 J/K•mol]
Determine if the photosynthesis reaction is spontaneous at 80°C. Chemical Equation: CO2 + H20 – C6H1206 + 02 Compound CO2 H20 C6H1206 02 AH° (kJ/mol) |-393.5 AS° (J/K•mol) 213.6 -285.8 69.9 |-1274.5 212.1 0 205 2. Compute for the AS° rxn ( J/K•mol) of the equation: (round off final answer to 1 decimal place)
The reaction, Fe203(s) + 3C(s) → 2Fe(s) + 3CO(g) AH° = +490.7 kJ, AS° = +541 J-K-1 %3D This reaction is spontaneous only below a certain temperature always spontaneous never spontaneous spontaneous only above a certain temperature
eq M M IS M ots M M M # 3 E D Consider the reaction 2H₂O(l) 2H₂(g) + O₂(g) The standard free energy change for this reaction is 474.2 kJ. The free energy change when 1.88 moles of H₂O(1) react at standard condition is kJ. 20 C What is the maximum amount of useful work that the reaction of 1.88 moles of H₂O(l) is capable of producing in the surroundings under standard conditions? If no work can be done, enter none. kJ Submit Answer $ 4 R F > % 5 T [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining G Cengage Learning Cengage Technical Support 6 B MacBook Pro Y Topics] H & 7 N U J ▶II * 00 8 M I ( 9 K. O < 96 ) L P V t Previous Email Instructor Save and Exit { + 11 [ Next ? } 1 dele
Gibbs free E 1
Using H° data, calculate the standard enthalpy change for the reaction at 298K. 2 NH3(g) HNO3(aq) --> NO2(g) 2 H20(1) AH° (KJ/mol) -46.19 -206.6 33.84 -285.83 (Note: the table AH values are located directly below the corresponding compound, this is the number found in the Appendix)
2 For the synthesis of ammonia where AG = -33.3 kJ/mole, determine whether the reaction is spontaneous at 25 C with the following pressures: PN, = 1.0 atm, PH, = 3.0 atm, PNH, = 0.020 atm N2(8) + 3H2(g) = 2NH3(g)
Use the following table to calculate ArH°, AS°, & A,Gº for the following reaction at 298K, then calculate it for -32°C and 250°C. 3 H₂ (g) + N₂(g) → 2 NH³(g) H₂(g) N₂(g) NH3(g) S°(J/K mol) 130.7 191.6 192.8 Which temperature(s) make the reaction spontaneous? AH (Kj/mol) 0 0 -45.9
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 74.0 °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. AH = 181. kJ AS = -499. K ? 2NO(g) N, (g) + 0, (g) AG = kJ Which is spontaneous? this reaction the reverse reaction neither