Is the reaction shown below spontaneous under standard conditions? (10 pts each)
P4O10(s)+16 H2(g) -> 4 PH3(g)+10 H2O(g)
Calculate Kp for this reaction.
Calculate ∆G if the amount of chemicals is adjusted to 5.6 g P4O10, 2 atm H2, 0.35 atm PH3, and 0.58 atm water?
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Is the reaction shown below spontaneous under standard conditions? (10 pts each) P4O10(s)+16 H2(g) -> 4...
a) Calculate Kp for this reaction. (10 pts each) P4O10(s) + 16 H2(g) -> 4 PH3(g) + 10 H2O(g) -) Calculate AG if the amount of chemicals is adjusted to 5.6 g P.0.0, 2 atm H2, 0.35 atm PH3, and 0.58 atm water?
Please write out equation used, indicate the values used or ICE tables, when necessary. 12) a) Is the reaction shown below spontaneous under standard conditions? P4010(s) + 16 H2(g) 4 PH3(g) + 10 H2O(g) b) Calculate Kr for this reaction. c) Calculate AG if the amount of chemicals is adjusted to 5.6 g P4010, 2 atm H2, 0.35 atm PH3, and 0.58 atm water?
Consider the reaction P4O10(s)+16 H2(g) -> 4 PH3(g)+10 H2O(g) Assume you have a container of the four components at equilibrium. What would happen to the amount of solid in the container if: )a) water was added. b) water was removed. c) the size of the container was decreased. d) internal pressure was doubled by adding He to the container. e) temperature of the container was increased.
Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) - 2 Fe(s) + 3 CO2(g) AG° = -28.0 kJ P(CO) - 3.1 atm, P(CO2) - 1.7 atm Calculate Arxn at 298 K, and indicate if the reaction is more or less spontaneous under these conditions than under standard conditions? -4.5 kJ, more spontaneous than under standard conditions None of these -4.5 kJ, less spontaneous than under standard conditions -23.5 kJ, more spontaneous than under standard conditions...
Under certain conditions, the reaction H2O(g) + C(s)=CO(g) + H2(g) is at equilibrium, and the Kp is 5. The partial pressure for H2O is 1.5 atm, for CO is 3.0 atm. What is the partial pressure of Hy in atm?
Please write out equation used, indicate the values used or ICE tables, when necessary. 13) Consider the reaction shown in 12 above. Assume you have a container of the four components at equilibrium. What would happen to the amount of solid in the container if: a) water was added. b) water was removed. c) the size of the container was decreased. d) internal pressure was doubled by adding He to the container. e) temperature of the container was increased. Is...
Calculate Grxn at 298 K under the conditions shown below for the following reaction. 2 H2S(g) + 3 O2(g) 2 SO2(g) + 2 H2O(g) G°rxn = ? G°f (kJ/mol) -33.4 -300.1 -228.6 P(H2S) = 1.4 atm, P(O2) = 0.5atm P(SO2) = 2.2atm and P(H2O) = 0.8 atm
The reaction A(g) B(g) is spontaneous under standard conditions. Which of the following statements are 1. The reaction B(g) → Alg) is nonspontaneous under standard conditions. II. Alg) will be completely converted to B(g) if sufficient time is allowed. III. Alg) will be completely converted to B(g) rapidly. A. I. only B. I. and II. only C. I., II. and III. D.I. and III. only E. II. only F. III. only
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
For the reaction: C(s) + H2O(g) CO(g) + H2(g), ΔH° = 131 kJ and ΔS° = 128 J/K at 298 K. At temperatures greater than ______ K, this reaction is spontaneous under standard conditions. a. 1.02 K b. 273 K c. 1023 K d. 753 K