Consider the following system at equilibrium where H° = 108 kJ, and Kc = 1.29×10-2, at 600 K: COCl2(g) CO(g) + Cl2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc fill in the blank 1 A. Increases     B. Decreases     C. Remains the same   The value of Qc fill in the blank 2 A. Is greater than Kc     B. Is equal to Kc     C. Is less than Kc   The reaction must: fill in the blank 3 A. Run in the forward direction to restablish equilibrium.     B. Run in the reverse direction to restablish equilibrium.     C. Remain the same. Already at equilibrium.   The concentration of Cl2 will: fill in the blank 4 A. Increase.     B. Decrease.     C. Remain the same

Consider the following equilibrium: N₂(g) + 3H₂(g)2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 9.24 atm of ammonia system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S

Consider the following system at equilibrium where H° = -18.8 kJ, and Kc = 10.5, at 350 K:2CH2Cl2(g) CH4(g) + CCl4(g)If the TEMPERATURE on the equilibrium system is suddenly increased: The value of Kc fill in the blank 1 A. Increases     B. Decreases     C. Remains the same   The value of Qc fill in the blank 2 A. Is greater than Kc     B. Is equal to Kc     C. Is less than Kc   The reaction must: fill in the blank 3 A. Run in the forward direction to restablish equilibrium.     B. Run in the reverse direction to restablish equilibrium.     C. Remain the same. Already at equilibrium.   The concentration of CCl4 will: fill in the blank 4 A. Increase.     B. Decrease.     C. Remain the same.

14. This is the third of three questions. Starting from 1.20 atm NOCI, 0.010 atm Cl₂ and 0.010 atm NO what is the value of AGO at 35 °C after equilibrium has been achieved? 2 NOCI(g) = 2 NO(g) + Cl₂(g) Kp = 1.6 x 10-5 at 35 °C Report your answer in kJ with as a whole number (the ones place), but do not write the units. Include a Your Answer: - if applicable.

Answer the following questions

For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25°C, it is found that the partial pressure of C is 0.270 atm. What is AG° for this reaction? (R = 8.314 J/mol · K). kJ/mol 1 3 4 C 7 8 9 +/- x 100 + 2.

Calculate the equilibrium constant, Kc, for the reaction: 2SO3(g) + 2SO2(g) O2 (g) Given the following data: a) initial conc. of SO3 (g) = 1.32 M b) Equilibrium conc. of SO3 (g) = 0.287 M c) initial conc. of SO2 (g) = 0.282 M d) initial conc. of O2 (g) =0.127 M