Given that -RT InK = H₂-H₂-TAS, if theequilibrium constant is 0.031 and H.-H, =44 kJ, what is the value of AS and 298.15 K?(R-8.314 J mol K')Select one:Oa 20.12 J KO b. 118.8 J KO c. 12.34 J KO d. 188.8 J K

The equilibrium constant is ....To find .

Given that -RT InK = H, -H, -TAS, if the equilibrium constant is 0.031 and H₁-H, - 44 kJ, what is the value of AS and 298.15 K? (R-8.314 J mol K') Select one: Oa 20.12 J K O b. 118.8 J K Oc 12.34 J K K O d. 188.8 J

Given that -RT InK = H, -H, -TAS, if the equilibrium constant is 0.031 and H₁-H, - 44 kJ, what is the value of AS and 298.15 K? (R-8.314 J mol K') Select one: Oa 20.12 J K O b. 118.8 J K Oc 12.34 J K K O d. 188.8 J

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

E D The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K. 80 PC13(g) + Cl₂(g) PCl5(g) If AH° for this reaction is -87.9 kJ, what is the value of Kp at 589 K? Kp Submit Answer 4 ? 000 000 R F DO LO % 5 Use the References to access important values if needed for this question. Retry Entire Group 7 more group attempts remaining T Cengage Learning Cengage Technical Support G < 6 Y H & 7 U J 8 I 9 K O 0 L P Previous Email Instructor Save and Exit + 11 Next { [ } ]
Consider the following system at equilibrium where AH° = -87.9 kJ/mol, and K. = 83.3 , at 500 K. PCI3 (g) + Cl2 (g) = PCI5 (g) When 0.22 moles of PCI3 (g) are removed from the equilibrium system at constant temperature: The value of Ke increase. decrease. remain the same. The value of Qc K.. is greater than is equal to is less than The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of Cl, will increase. decrease. remain the same.
To manufacture S03 with the reaction 2S02(g) + 02 - > 2S03(g) A H° = -99 kJ, one way to increase the equilibrium S03 would be to O decrease oxygen O decrease SO2 increase pressure increase temperature
reg # 3 [Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = 108 kJ, and K. = 1.29 × 10-2, at 600 K: COC1₂ (g) CO(g) + Cl₂ (g) E 20 If the temperature on the equilibrium system is suddenly increased: The value of Ke D Oincreases Odecreases O remains the same The value of Qc Ols less than Ke Ois greater than K O is equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of Cl₂ will Oincrease Odecrease Oremain the same Submit Ans Show Hint $ 4 000 000 F4 R F % 5 T ry Entire Group Cengage Learning | Cengage Technical Support G A 6 9 more group attempts remaining MacBook Air Y H & 7 U * 00 8 ( 9 K O -0 ) F10 P 4) F11 Previous + 11 Next> Save and Ex A
The Haberprocess is exo thermic. Cthe formation of NH3 from its elements) a) wribe out the balanced Chemical equation (with subscripts) and include energy b) If you were to maximile product yiel, would increase or decrease heat you to the system? c) Explain what stress could have caused the changes the graph below N2 equilibrium reached NH, Concentration (mol/L)
10:26 1 4 7 +/- For the reaction 2 A (g) → B (g), Kp = 0.00617 at 298 K. When AG = 8.35 kJ/mol, what is the partial pressure of B when the partial pressure of A is 2.00 atm for this reaction at 298 K. 2 5 Question 12 of 15 8 atm 3 6 9 0 al 9% Tap here or pull up for additional resources ||| O Submit Xx C x 100
Consider the following system at equilibrium where AH° = -87.9 kJ, and K. = 83.3, at 500 K. PC13(g) + Cl2(g) =PCI5(g) When 0.31 moles of Cl2(g) are removed from the equilibrium system at constant temperature: The value of K. increase. decrease. remain the same. The value of Qc K.. is greater than is equal to is less than The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of PC13 will increase. decrease. remain the same.
For the reactionCH4(g) + 2O2(g)CO2(g) + 2H2O(g)H° = -802 kJ and S° = -5.20 J/KThe equilibrium constant, K, would be greater than 1 at temperatures (above,below) (___) ___Kelvin.Select above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant. ---- For the reactionHCl(g) + NH3(g)NH4Cl(s)H° = -176 kJ and S° = -285 J/KThe equilibrium constant, K, would be greater than 1 at temperatures (above,below) (___) ____Kelvin.Select above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant.
ient/takeCovalentActivity.do?locator-assignment-take Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x102, at 1.15x10° K. 2S03(g) 2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value ofK. A. increases. B. decreases. C. remains the same. The value of Q. A. is greater than K.. B. is equal to K. C. is less than K. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of O, will: A. increase. B. decrease. C. remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Prev