Calculate AG for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) when...
Calculate Δ G for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) when P of SO2 = 0.500 atm, P of O2 = 0.0100 atm, and P of SO3 = 0.100 atm. The value for Δ G^o for this reaction at 298 K is -141.6 kJ. ΔG = ???? kJ I got -160.9 kj but it is incorrect.
Calculate AG for the reaction 2 So, (e)+0,() + 250, (e) when P of so,=0.500 atm, Pof O2 = 0.0100 atm, and Pof So, = 0 100 atm. The value for AGº for this reaction at 298 K is -141.6 kJ AG= Is this reaction spontaneous or non-spontaneous under these conditions? Spontaneous or non-spontaneous?
Calculate AG for the reaction 2 50,000,00) reaction at 298 K is - 141.6 kJ Due in 1 hours, 29 minutes Due Sun 11/17/2019 11:59 pm 250, c) when Pof so, -0.500 atm. Pof O, 00100 m, and Pof so, - 0100 m. The value for AG" for the AG - Is this reaction spontaneous or non-spontaneous under these conditions? Spontaneous or non-spontaneous
For the reaction 2 SO2(g) + O2(g) →→2 SO3(g) AG° = -140.3 kJ and AS = -187.9 J/K at 306 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 306 K. The standard enthalpy change for the reaction of 1.79 moles of so,(g) at this temperature would be
5) For the reaction 2 SO2(g) + O2(g) → 2 SO3(g), if initially P(SO2) = 1.2 atm, P(O2) = 1.8 atm, and P(SO3) = 2.1 atm, calculate AG for this reaction at 25°C. The following data is valid at 25°C: AG° (kJ/mol) SO 300.4 SO3 370.4 A) -140.0 kJ/mol B)-141.3 kJ/mol C)-138.7 kJ/mol D) 1,174.7 kJ/mol E) -137.6 kJ/mol
a) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g): 2. 2SO2(g) O2(g)SO3(g) dGo, ΔΗο, and ASo values for the reaction are-141 .6kJ/mol,-1984kJ/mol and -187.9J/Kmol, respectively. Evaluate whether or not the reaction is spontaneous under standard conditions at 298K, predict the effect of increasing temperature on spontaneity and calculate the value of T at which the reaction becomes nonspontaneous. b) The reaction described in part (a) is too slow at room temperature to...
Calculate Kp at 298 K for the reaction SO.(g) + NO2()SO3(g)+NO() SO2(g) SO3(g) NO(g) NO2(g) -300.4 k/mol -370.4 kJ/mol 86.7 kJ/mol 51.8 kJ/mol For the reaction 2NO(g)+02(g)- 2NO2( f iniially P(NO)1.5 atm, PO2)-1.4 atm, and P(NOJ-2.0 atrn, calculate Δ@for this reaction at 25°C. The following data is valid at 25°C: NO NO2 AGe(kJ/mol 86.7 51.8
Consider the reaction: 2 POC13 (g) → 2 PC13 (g) + O2(g) a) Calculate AG. for the reaction (AH. = 572 kJ; AS = 179 J/K) at 298 K. b) Is the reaction spontaneous or not spontaneous? At what temperature would it reach equilibrium?
Given the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Starting with 0.100 M of SO2 and 0.050 M of O2, which value of K should be used and why? a. KC because the chemicals are in the gas phase. b. KP because the concentrations are in Molarity. c. KP because the chemicals are in the gas phase. d. KC because the concentrations are in Molarity.
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