a) Calculate Kp for this reaction. (10 pts each)
P4O10(s) + 16 H2(g) -> 4 PH3(g) + 10 H2O(g)
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a) Calculate Kp for this reaction. (10 pts each) P4O10(s) + 16 H2(g) -> 4 PH3(g)...
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?
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 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?
(a) Calculate ∆G for the reaction: C(s, graphite) + H2O (g) ↔ CO (g) + H2 (g) where temperature is 700 K, ∆G⁰ = 92 kJ and the initial pressure of each gas is P H2O = 0.67 atm, P CO = 0.23 atm, P H2 = 0.51 atm. (b) What direction would this reaction proceed?
1 pts Question 10 For the reaction P4O10(s) + 6H2O)® 4H3PO4(aq), what mass of P4O10 must be consumed if 3.71 1023 molecules of H2O are also consumed? 66.6 g 29.1g 175g 1050 g O 1.85 g
The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO=1.15 atm, and PH2= 1.45 atm? Part A What is the equilibrium partial pressure of H2O? Part B What is the equilibrium partial pressure of CO? Part C What is the equilibrium partial pressure of H2?
Consider the reaction 4 PH3(g) → P4(g) + 6 H2(g). If, in a certain experiment, over a specific time period, 0.0045 mole of PH3 is consumed in a 1.7-L container during each second of the reaction, what are the rates of production of P4 and H2 in this experiment? P4 mol L−1 s−1 H2 mol L−1 s−1
The equilibrium constant Kp for the reaction C(s)+H2O(g)⇌CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO= 1.30 atm, and PH2= 1.40 atm? Part A What is the equilibrium partial pressure of H2O? What is the equilibrium partial pressure of CO? What is the equilibrium partial pressure of CO?
Cls, graphite)+H2O (g)CO (B)+H2 (g) (a) Calculate AG for the reaction: where temperature is 700 K, AG° 92 kJ and the initial pressure of each gas is P H,0 = 0.67 atm, P co 0.23 atm, P H, = 0.51 atm. (b) What direction would this reaction proceed?