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Problem 4 The value of Δ110 is-12.93 kJ mol-1 for the following reaction: 2HI(g)H2(g) +12(9) Assuming...
b) General chemistry textbooks often show this simplified derivation of the van't Hoff equation A, G In Kp - dln K Then, under the assumption that Д.Ho and Δ,So are independent of temperature dln K, However, the Gibbs-Helmholtz equation and, correspondingly, the van't Hoff equation, is a general re- lationship that gives the proper expression for the derivative of Kp at a specific temperature even when ΔΤΗ"and Δ,So are functions of temperature, i.e., when Δ7"Ho Δ,Ho(T) and Δ,So-Δ7S®(T) Show, directly...
ΔGf°(I2(g)) = 19 kJ/mol 7. For the reaction H2(g) +12(g) = 2HI(g) K = 50.0 at 721 K (a) What is AG at 721 K? (b) What is Kat 25 °C? (AG HI(g) = +1.7 kJ/mol)
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all speies. For the reactionC2H6(g)+H2(g)↽−−⇀2CH4(g)the standard change in Gibbs free energy is Δ𝐺∘=−32.8 kJ/mol.ΔG°=−32.8 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are 𝑃C2H6=0.400 bar,𝑃H2=0.150 bar, and 𝑃CH4=0.850 bar?𝑃CH4=0.850 bar? Δ𝐺=_____ kJ/molSk
A,) ΔG o for the reaction H2(g) + I2(g) ⇌ 2HI(g) is 2.60 kJ/mol at 25°C. Calculate ΔG, and predict the direction in which the reaction is spontaneous. The initial pressures are: PH2 = 3.10 atm PI2 = 1.5 atm PHI 1.75 atm ΔG = kJ/mol b.)The reaction is spontaneous in the forward direction. The reaction is spontaneous in the reverse direction. Cannot be determined.
For the reaction H2(g)+I2(g)⇌2HI(g), K= 57.0 at 700 K what can be said about this reaction at this temperature? For the reaction , at 700 what can be said about this reaction at this temperature? The equilibrium lies far to the right. The reaction will proceed very slowly. The reaction contains significant amounts of products and reactants at equilibrium. The equilibrium lies far to the left.
H2(g) + I2(g) ⇌ 2HI(g) ΔG o for the reaction is 2.60 kJ/mol at 25°C. What is the minimum partial pressure of I2 required for the reaction to be spontaneous in the forward direction at 25°C if the partial pressures of H2 and HI are 4.1 and 2.05 atm, respectively?
please help!!!! For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° = -176.6 J/mol K. What is AG for the reaction at 45.0°C when P_NO2 = P_N204 = 0.200 atm? Assume AH° and ASº are temperature independent. ple For the electrochemical cell 2 Al(s) + 3 Mn2+(aq) + 2 Al3+ (aq) + 3 Mn(s) (E° = 0.48 V, [A13+] = 1.0 M), what is the value of E when [ Mn2+] = 0.016 M? Assume Tis...
1) Calculate 4G rx (350 K) for the reaction: H2O(g) +0.502(g) → H2O2(1) using the Gibbs-Helmholtz equation and (46°F 2120-228.57 kJ/mol; 4G°F (H202)-120.35 kJ/mol; Hºr ano)-241.82 kJ/mol; AHF (H202)=-198.78 kJ/mol). You may assume that the difference between 4GºrxN and AHørxn is temperature independent.
NOLUL PULS. AGº for the reaction H2(g) +12(8) = 2HI(g) is 2.60 kJ/mol at 25°C. Calculate AG, and predict the direction in which the reaction is spontanec The initial pressures are: PH, = 3.70 atm P1, = 1.5 atm Ph1 = 1.75 atm AG= The reaction is spontaneous in the forward direction. The reaction is spontaneous in the reverse direction. Cannot be determined.
9. The equilibrium constant for the reaction H2(g) + I2(g) 2HI(g) has a value of 54.6 at 699K. What are the equilibrium concentrations of H2, I2, and HI if the initial concentrations at this temperature are 0.0800M H2 and 0.0700 M I2. 10. Find the pH and pOH of a solution prepared by dissolving 9.85 grams of NaOH into a total aqueous solution volume of 75.0 ml. 11. Using the data in Appendix B of your text, calculate the values...