dG = dH - TdS ( from 2nd law of thermodynamics)
since reaction is taking place at standard condition hence T = 273 K
therefore
dG = 1900 - (273 * (-109) ) = 31657 J/mol or 31.657 kJ/mol
(since 1kJ = 1000 J)
Question 13 1 pts Determine 4Gºrxn using the following information, H2(g) + CO(g) -CH2O(g) AH°= +1.9...
Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K (Hint- What is the temperature when measuring standard heat of energy and change in entropy)
Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K (Hint- What is the temperature when measuring standard heat of energy and change in entropy)
Determine the equilibrium constant for the following reaction at 459 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) AH° = -94.9 kJ; AS°= -224.2 J/K
Determine the equilibrium constant for the following reaction at 459 K. CH2O(g) + 2 H2(g) - CH4(g) + H2O(g) AH° = -94.9 kJ; AS°= -224.2 J/K 1.44 x 10-2 1.23 2.08 x 10-3 35.07 x 10-4 122x 10-1
8) HY 8) Consider a reaction that has a negative AH and a positive AS. Which of the following statements is true? A) This reaction will be spontaneous only at high temperatures. B) This reaction will be spontaneous at all temperatures C) This reaction will be nonspontaneous at all temperatures. D) This reaction will be nonspontaneous only at high temperatures. E) It is not possible to determine without more information 9) What is the volume of 5.60 g of O2...
1.(3pts) Use the following data to determine the AH... of 2 CH2O(1) + 15 O_() ---> 10 CO(g) + 12 H.O(1) Data: Substance AH(kJ/mol) Substance AH(kJ/mol) CHg) CH,OH(L) C.H.O(1) CH401) H2O(g) CO(g) O2(g) 20.9 -239.0 -277.0 -316,0 -241.82 -110.53 CH.(8) CH,OH(S) CsH 20 (1) CHO(1) HO() -104.0 -201.0 -298.6 -340.0 -285.83 -393.51 CO2 NB) 2.(2pts) If you are given 148.0 g O(g) and a sufficient amount of the other reactant, calculate the heat associated with reaction in problem 1 and...
Question 8 of 20 Using the equations H2(g) + F2 (g) → 2 HF (g) AH° = -79.2 kJ/mol C(s) + 2 F2 (g) → CF. (g) AH° = 141.3 kJ/mol 2 C(s) + 2 H2 (9) C2H4 (9) AH = -97.6 kJ/mol Determine the enthalpy for the reaction C2H4 (g) + 6 F2 (g) → 2 CF4 (9) + 4 HF (g). kJ/mol
For the reaction CO(g) + H2O(1)—*CO2(g) + H2(g) AH° = 2.8 kJ and AS° = 76.8 J/K The standard free energy change for the reaction of 2.33 moles of CO(g) at 288 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 288 K. Assume that AH° and ASº are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining For the reaction 2 NO(g) + O2(g) → 2 NO2(g) AG°...
1.(3pts) Use the following data to determine the AH of > 8 CO (g) +5 H2O() 2 C Hiog) +13 O2(g) AH (KJ/mol) Substance AH (kJ/mol) Substance Data: -104.0 CaH&(g) CHHОН() CH12(g) CH&(I) НО) Со N2(g) С.Н.8) CH2OH(I) -239.0 C&Hio(g) C&H12(I) H2O(g) CO(g) O2(g) 20.9 -201.0 -146.44 -126.15 +12.0 -156.4 285.83 -241.82 -393.51 -110.53 0
13. Consider the following equation 2 C(s) + 2 H2O(g) + CH, (g) + CO2(g) Determine the standard enthalpy change for this reaction from the following standard enthalpies of reaction : (1) C(s) + H2O(g) + CO(g) + H2(g) AH° = 131.3 kJ (2) CO (g) + H2O(g) + CO2(g) + H2(g) AH° = -41.2 kJ (3) CH, (g) + H2O(g) + 3H2(g) + CO (g) AH° = 206.1 kJ A. 15.3 B. -116.1 C. 378.2 D. -427.0