Consider the following system at equilibrium where AH = 18.8 kJ and K = 0.0952, at 350. K. CH₂(g) + CCL (9) 2CH₂Cl₂ (9) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of Ke Oincreases O decreases Oremains the same The value of Qe Ois greater than Ke O is equal to Ke O is less than Ke The reaction must Orun in the forward-direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. Oremain the same. It is already at equilibrium. The number of moles of CC14 will Oincrease Odecrease Oremain the same

The chemical equation for an equilibrium is described below. kJ mol CaO (s) + CO2(g) = CaCO3(s) AH° Predict how the following changes would shift the equilibria. Be sure to start by writing the equilibrium (K) equation. =-176-

Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(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 Q 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 reestablish equilibrium.     B. run in the reverse direction to reestablish equilibrium.     C. remain the same. It is already at equilibrium.   The concentration of H2 will: fill in the blank 4 A. increase.     B. decrease.     C. remain the same.

[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. 77.5, at 600 K. CO(g) + C,(g) COCI,(g) When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish cquilibrium. O remain the same. It is already at cquilibrium. The concentration of CO will Submit Answer Retry Entire Group 1 more group attempt remaining

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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

When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H2O(g) <--> CO2(g) + H2(g) +heat  For each of the following changes at equilibrium, indicate whether the equilbrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) (d) adding more H2O(g) (e) decreasing the volume of the container

[References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 16.1 kJ, and Kc = 6.50 x 10-3, at 298 K: 2NOBr(g) 2NO(g) + Br₂(g) If the VOLUME on the equilibrium system is suddenly increased at constant temperature: The value of Ke Oincreases O decreases O remains the same The value of Qc O is greater than Ke O is equal to Ke O is less than K The reaction must run in the forward direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. Oremain the same. It is already at equilibrium. The number of moles of Br2 will O increase O decrease O remain the same Show Hint F5 6 H F6 & 7 KI F7 * 8 DII F8 ( 9 DD F9 ) O F10 P F11 Previous + Next Save and Exit F12 delete

For the equilibrium system below, which of the following would result in an increase in the quantity of H₂(g)? H₂(g) + 12(g) 2HI(g) + 65 kJ ос removing some I₂(g) and removing some HI(g) removing some HI(g) removing some 1₂(g) decreasing temperature removing some HI(g) and decreasing temperature

Consider the following equilibrium: 2NO, (g)–N,04 (8) AGº= – = - 5.4 kJ Now suppose a reaction vessel is filled with 5.06 atm of dinitrogen tetroxide (N,0) at 400. °C. Answer the following questions about this system: 2 rise Under these conditions, will the pressure of N,0, tend to rise or fall? 2 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can yes that be changed to a tendency to fall by adding NO,? Similarly, if you no said the pres of N,0, will tend to fall, can that be changed to a 2 4 tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, needed to reverse it. atm Round your answer to 2 significant digits.