NO2(g) ⇌ N2O4(g) Kp = 11.3 at 25oC (a) Calculate G if the P(NO2) = 0.29 atm, and...
NO2(g) ⇌ N2O4(g) Kp = 11.3 at 25oC
(a) Calculate G if the P(NO2) = 0.29 atm, and P(N2O4) = 1.6 atm.
(b) Predict the direction in which the reaction will shift to reach equilibrium. Explain how you determined this.
(c) Once equilibrium is reached are there more reactants or products present. Explain how you determined this.
Homework Answers
![kp=113 at es c. NO(g) - HQOA (8) iTo 95c : 298k. AG°E-RT nk. AG = AGO + RT ln Q. PLM22] = 1-6 afm. a) Given- PLNO2] = 0.29cm](http://img.homeworklib.com/questions/fd59a3e0-4d0d-11ec-8978-ada394eb1df3.png?x-oss-process=image/resize,w_560)
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NO2(g) ⇌
N2O4(g) Kp
= 11.3 at 25oC
(a) Calculate G if the P(NO2) = 0.29
atm, and...
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A flask is charged with 1.500atm of N2O4(g) and 1.00 atm NO2(g) at 25 degree C, and the following equilibrium is achieved: N2O4(g) 2NO2 After equilibrium is reached, the partial pressure of NO2 is 0.519atm. Calculate the value of Kp for the reaction. Calculate Kc for the reaction.
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1) At 298 K, an equilibrium
mixture contains P H2=0.958 atm, P I2= 0.877 atm and P HI=0.020
atm. Please try and answer all!
You must show all your work to receive credit. Watch sig figs! Consider the reaction: 1) At 298 K, an equilibrium mixture contains P H2-0.958 atm, P ½=0.877 atm, and P HI-0.020 atm. Calculate the value of the equilibrium constant Kp? a) (o, o2) 0.938x o.87? b) And what is the value of the equilibrium constant...
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