Consider the following system at equilibrium where H° = -16.1 kJ, and Kc = 154, at 298 K.2NO(g) + Br2(g) 2NOBr(g)If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of Kc   A. increases.     B. decreases.     C. remains the same.   The value of Qc   A. is greater than Kc.     B. is equal to Kc.     C. is less than Kc.   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 Br2 will:   A. increase.     B. decrease.     C. remain the same.

Consider the following equilibrium: 2NO₂ (g) N₂O₂(g) AG=-5.4 kJ Now suppose a reaction vessel is filled with 0.316 atm of nitrogen dioxide (NO₂) at 708. "C. Answer the following questions about this system: Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O₂? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O₂ needed to reverse it. Round your answer to 2 significant digits. rise O fall O yes O no atm 0.8 X

Nitric oxide reacts with chlorine to form NOCI. 2NO(g) + Cl2g) → 2NOCI(g) The equilibrium constant K at 298K is x 107. (R = 8.314 J/K • mol) Substance: NO(g) Cl2g) NOCIG) AH°F (k]/mol) at 298 K 90.29 51.71 S°U/K• mol) at 298 K 210.65 223.0 261.60

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.

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.

An aqueous solution of a particular compound has pH =7.46. The compound is O a weak base O a weak acid a strong acid O a strong base

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