Find AG (in kJ mol-1 to one decimal place) for the following reaction at 198.15 K...
Find AG (inkJ mol 1 to one decimal place) for the following reaction at 198.15K when РН= 3.0 atm, PH2= 1.0 atm, and P2-4.0 atm. Нs) + 1 (8) ӘНІ(8) О 58 o 2.6 о 0.2 06.1 о -5.8 O 54 o 34 о -1.2 o 21 0 0.6 O 1.2 o o o
8. The AG for the reaction H2(g) + 12(e) = 2 HI) is 2.60 kJ/mol at 25°C. In an experiment, the initial pressures are Pe = 3.98 atm, P = 0.044 atm, and P = 0.29 atm. Calculate AG for the reaction and predict the direction of the net reaction
Calculate ΔGrxn (in kJ/mol with 1 decimal place) for CH3OH(g) ↔ CO(g) + 2 H2(g) at 25ºC given PCH3OH= 0.855 atm, PCO= 0.125 atm, PH2= 0.357 atm.
At 699 K, AG° = -23.25 kJ for the reaction H2(g) + 12(g) = 2 HI(g). Calculate AG for this reaction if the reagents are both supplied at 10.0 atm pressure and the product HI is at 1.00 atm pressure. Select one: O a. -36.6 kj O b. -50.0 kj O C. -3.5 kg O d. +50.0 kJ o e. +36.6 kJ
AH = 44.0 kJ/mol AS = 0.119 kJ/mol K The following reaction takes place at 120°C: H20(1) - H2O(g) Which of the following must be true? Select one: O a. Two of these O b. The reaction is not spontaneous O c The reaction is spontaneous. O d. AG = 0 e. AGO
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 = 1.83 bar PSi2H6 = 0.96 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). ΔGf(Si2H6) = 127.3 kJ/mol ΔGf(H2) = 0 kJ/mol
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.
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6 (g) The conditions for this reaction are: PH2 = 1.15 bar PSi2H6 = 0.17 bar
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) The conditions for this reaction are: PN2 = 1.47 bar PH2 = 0.35 bar PNH3 = 1.45 bar
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)