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help me find delta g 3. Calculate AG for this reaction at 500.°C. AH = -92...
1. Calculate AG°for the following reaction at 25°C using AG ° = AH ° - TAS° Fe2O3 (s) + 3 H2(g) → 2 Fe (s) + 3 H2O (1) 2. Calculate AG ° for the same reaction using AG°f values Fe2O3 (s) 3 H2(g) → 2 Fe (s) + + 3 H20 (1) + 3. Calculate AGº of the following reaction: 2C (s) H 2 (g) → C2H 2 (g) Use Hess' Law, AG° = AG°1 + AG°2 + AG°3...
Consider the reaction of NO(g) from its elements. 2 502(g) + O2(g) → 2 SO3(9) Use the thermodynamic data given to determine the following for this reaction: AH°, equal O kJ/mol Asº, equals O J/molk Calculate the AG, at 500 °c with all gases at standard pressure and equilibrium constant K at 500 °C. AG, at 500 °c equals O kJ/mol K at 500 equals tance (kJ/mol) (J/mol-K) O2(g) 205.2 SO2(g) -296.8 248.2 SO3(9) -395.7 240.0 AHO so
AG°= AH-TAS AG=AGº+RTinQ where R=8.314 J/mol K 1. Calculate AGº for the following reaction at 25 °C if AH°= -1854 kJ/mol; AS°= -236 J/mol K CH-COCH3(g) + 402(g) → 3C02(g) + 3H2O(1) 2. NH.NO, dissolving in water is a spontaneous process. As it dissolves, the temperature of the solution decreases. Based on this, what must the signs (positive or negative) of AG, AH, and AS be?
9) Using the information given calculate, AH, AS and AG at 25°C (remember, for a reaction calculated using the relationship: AH = AH° reaction = nАHºf(products) - EnАHºt(reactants). PAY ATTENTION TO UNITS AND SIGN PC13(g) + Cl2 (g) → PCls(g) AHºt(kJ/mol) -287 O -374.9 (why is AHºt = 0 for Cl2?) Sºt (J/K) 311.67 223.1 364.47
Question 5 Correct Use AG° =AH° -TAS° to calculate AG (in kJ) at 298 K for : Mark 1.00 out of 1.00 2002(g) +4H2O(1) ► 2CH3OH(1) + 302(g) P Flag question Answer: 1404.84 Question 6 Not answered Marked out of 1.00 If the above reaction could be done at 3399 K, what would be your estimate for AGº (in kJ) at this elevated temperature? Use AGⓇ =AH°-TAS and assume AH° and AS are independent of temperature. P Flag question (Theis...
For a particular reaction, AH = -14.20 kJ/mol and AS = -198.5 J/(mol.K). Calculate AG for this reaction at 298 K. AG = 73.35 kJ/mol
Using provided data, determine AG* (in kJ) for the following reaction. 2036) ++3026) AH,(kJ/mol) S /mol) Ozle) 205.0 Ole) 143 238.82 Question 11 2 pts Use the provided information to determine the equilibrium constant at 298 K for the reaction given 2NO26) N204(8) 4 AH® (kJ/mol) 5° (J/molk) NO2(g) 33.2 239.9 N2048) 9.16 304.3 Equilibrium Constant - (Select) x 10 (Select)
• Calculate AH , AS and AG for the reaction below at 115°C. Before you begin calculating, predict signs (+ or -) for enthalpy, entropy, and free energy of reaction. • Is the reaction spontaneous at 115°C? Na 0 (8) + H2O() → NaOH () Na,0 (s) HO (D) NaOH (s) AH°, (kJ/mol) 414.2 -285.8 -427.0 Sº (J/K-mol) 75.1 70.0 64.0
Calculate the AH for the following reaction: TICI4 (g) + 2 H20 (g) →TiO2 (s) + 4 HCI (8) compound AH+ (kJ/mol) TICIA -763 H20 -242 -945 HCI -92 TIO2 -66 kJ/mol +32 kJ/mol 0 -32 kJ/mol +66 kJ/mol -2.0 x 103 kJ/mol Question 27
Calculate Ksp for Ag2S(s), then calculate molar solubility of Ag+ and S2-. Delta G of Ag2S = -40.7KJ/mol Delta G of Ag+ = 77.11KJ/mol Delta G of S2- = 83.7KJ/mol ICE table and clear breakdown of relationship of Ksp and Delta G. please.