Photosynthesis in plants concerts carbon dioxide and water into glucose (CH1;Oa) and oxygen accordingto the equation below.6CO, (g) + 6H;0 (1)CHzO. (s) + 60, (g)Substanceco, (g)H,O (1)CHOs (s)O, (g)AH? (KJ/mol)-393.5-285.8-1 273.3S°(J/mol.K)213.669.9209.2205.0Calculate the AH°, AS°, and AG°, Is the reaction spontaneous at standard conditions?

Photosynthesis in plants concerts carbon dioxide and water into glucose (C,H1,O) and oxygen according to the equation below. 6CO, (g) + 6H;0 (1) CH,O, (s) + 60; (9) co, (g) H,0 (1) CHO, (s) O, (g) Substance AH? (KJ/mol) -393.5 -285.8 -1 273.3 S°(J/mol.K) 213.6 69.9 209.2 205.0 Calculate the AH°, AS°, and AG°, Is the reaction spontaneous at standard conditions?

Photosynthesis in plants concerts carbon dioxide and water into glucose (C,H1,O) and oxygen according to the equation below. 6CO, (g) + 6H;0 (1) CH,O, (s) + 60; (9) co, (g) H,0 (1) CHO, (s) O, (g) Substance AH? (KJ/mol) -393.5 -285.8 -1 273.3 S°(J/mol.K) 213.6 69.9 209.2 205.0 Calculate the AH°, AS°, and AG°, Is the reaction spontaneous at standard conditions?

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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2. Consider the combustion of methane (CH4) CHO) + 202(9) CO2(9) + 2H2O9) Calculate the AH°rxn- AH°; CH4(2) = -74.9 kJ/mol; AH°; CO2(e) = -393.5 kJ/mol; AH°f H2O(g) = -241.8 kJ/mol
Photosynthesis in plants converts carbon dioxide and water into glucose (C,H12O) and oxyge- according to the equation below. 1. 6CO,(g) + 6H,0(1) CH1,0(s) + 60,(g) Substance CO,(g) H,O() C,H12O6ls) Ozlg) AH?(kJ/mol) -393.5 -285.8 -1 273.3 S°J/mol · K) 213.6 69.9 209.2 205.0 Calculate the AH°, Asº, and AGº. Is the reaction spontaneous at standard conditions?
9. Use the standard enthalpies of formation in the table to answer the questions below Compound AH`; (kj/mol) Compound AH, (kJ/mol) CO(g) CO:(g) H2O(1) Fe:O2(s) -110.4 -285.8 -393.7 -822.2 a. Calculate the standard enthalpy of reaction for the equation Fe,O;(s) + 3 CO (g) → 2 Fe(s) + 3 CO2(g) b. The standard enthalpy of reaction for the equation below is -3535 kJ. Calculate the enthalpy of formation of CsH,2(1). C;H12(1) + 802(g) → 5 CO:(g) + 6 H20(1)
2. Given: C;H>(g) + 5/2 O2(g) → 2 CO2(g) + H2O (g) C (s) + O2(g) → CO2(g) H2(g) + ½ O2(g) → H2O (g) AH = -1220.6 kJ/mol AH = -503.5 kJ/mol AH = -103.8 kJ/mol Calculate the enthalpy for the following reaction: 2 C (s) + H2(g) → C¿H2(g)
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2. Calculate the AH for the reaction S +Olo) using these two reactions: + O, AH = -296.8 kJ 2(g) 2S03 (a) AH = -197.0 kJ 2S0, 21g) 2(g)
Please use the values in the resources listed below instead of the textbook values. Calculate the values of E°, A„G°, and K for the following reactions at 25.00°C. (Assume R = 8.3144621 J/mol·K. For each K, enter an unrounded value. Due to the nature of this problem, do not use rou intermediate values in your calculations-including answers submitted in WebAssign.) (a) Cu2+ + Pb - Cu + Pb2+ E° = 4.0 .467 V A,G° 4.0 -90.1 kJ•mol-1 K = 7.901e15 (b) Br2 + 2 I- → 2 Br¯ + I2 E° = 4.0 .550 V A,G° 4.0 -106 kJ•mol-1 K = 4.01e18 (c) 5 Cu+ + 8 H+ + MnO4¯ 5 Cu2+ + 4 H20 + Mn2+ E° = 4.0 1.36 V A,G° 4.0 -656 kJ•mol-1 K = 1.011e115
Given the heat of formation of the following compounds from their elements: AH°F = -393.5 kJ/mol AH°f = -285.9 kJ/mol CH;OH(1) AH°F = -238.6 kJ/mol CO((g) H;O(1) What is the value of AH® for the reaction; CH;OH() + 3/2 O:(2) – CO.(g) + 2 H;O(1) A) -726.7 kJ B) -416.9 kJ C) -346.2 kJ D) -440.8 kJ E) -1203.9 kJ
Determine AH for the combustion of 25.0 mL of C12H26(U) in excess O2 to give CO2(g) and H20(g). The density of C12H26 is 0.750 g/ml. Substance AH, (kJ/mol) C12H26(1) -353 Co:(g) -393.5 H2O(g) -241.8
What is DH°rxn (in kJ) for the reaction - CH4(g) + 202(g) · CO2(g) + 2H,0(1). --> DH°; (CH4(g)) = -74.8 kJ/mol DH° (CO2(g)) =–393.5 kJ/mol DH°F (H2O(1)) = -285.5 kJ/mol
Using data for DHof (KJ/mol) provided below, calculate DHoRxn for: N2O(g) + 3H2(g) ---> N2H4 (l) + H2O (l) DHof (KJ/mol): N2O(g) = 33.85 ; H2 (g)= 0 ; N2H4 (l)= 50.4 ; H2O(l) = -285.8