The reaction A2 + B2 2 AB has an equilibrium constant of Kc = 4 For each of the parts below, where A is shaded and B is unshaded: i. Determine if the reaction is at equilibrium, by calculating Q. If the reaction is not at equilibrium, predict which direction the reaction ii. would proceed to reach equilibrium (i.e. towards the products or towards the reactants). ji. Explain why this would happen. iv. If we draw a graph of AG vs Reaction Progress what would that look like? a.

00 II O KINETICS AND EQUILIBRIUM Using the van't Hoff equation to predict K at a different... At -18.7 °C the pressure equilibrium constant K, =7.2 for a certain reaction. d. Here are some facts about the reaction: -1 -1 • The initial rate of the reaction is 13. mol·L s . • Some of the reactants are liquids and solids. • If the reaction is run at constant pressure, 79.0 kJ/mol of heat are absorbed. O Yes. x10 Using these facts, can you calculate K, at -5.6 °C? No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K. will be d. bigger. If you said no, can you at least decide whether K, at Yes, and K, will be d. smaller. - 5.6 °C will be bigger or smaller than K, at – 18.7 °C? No. Explanation Check Terms of Use I Privacy Center A O 2021 McGraw Hill LLC. All Rights Reserved. DD F10 O00 F5 F4 esc F1 24 41 %23 6 7. 3.

At a particular temperature a 2.00 L flask at equilibrium contains 2.80 x 104 mol N2, 2.50 x 10-5 mol O2, and 2.00 x 10-2 mol N2O. The 2 N2(9) + Oz(9) = 2 N¿O(g) chemical reaction is: b. Calculate the equilibrium concentration of all the gases. c. Calculate the Keq.

1. Sulfur trioxide decomposes spontaneously to form sulfur dioxide and oxygen gases according to the following balanced equation: 2SO, 2SO2 w + O2 Under certain conditions, the equilibrium constant for the reaction is 6.9 x 107. What concentration of oxygen can be expected when 0.400 mol of SO,, comes into equilibrium in a 2.00-L vessel? a. 360 b. Is this mixture at equilibrium? In a 1.00-L container is placed 0.10 mol ofO, 0.50 mol of SO, and 0.20 mol of SO, If not, predict in which direction the reaction will shift. An equilibrium mixture of the same three gases is combined with 0.10 mol of Ar reaction responds by producing more SO, The c. 3 Explain this new equilibrium shift. d. Describe how might a sulfur trioxide manufacturer try to minimize this decomposition reaction? Please choose a method different from part c.

Consider the following system at equilibrium at 350 K: CHĄ(g) + CC4(g) =2CH,C2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: A. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The number of moles of CCl4 will: |A. Increase. B. Decrease. C. Remain the same.

Oxygen and ozone are allowed to come to equilibrium in the exothermic reaction 203(g) =302(g) Which change will increase the numerical value of the equilibrium constant, K? Periodic Table and Datasheet Select one: O a. adding more O2(g) O b. adding a suitable catalyst O c. decreasing the temperature O d. increasing the volume of the container

Given the Equilibrium Equation: CO (g) + Cl2 (g) <--> COCl2 (g) and ΔH = -25.9 kcal/mole Which option would make the equilibrium shift towards the products? Pick all that apply. (There may be multiple answers that are correct) a. adding more phosgene b. adding more carbon monoxide c. increasing the temperature d. decreasing the reaction container volume e. decreasing the temperature

Consider the following system at equilibrium at 648 K:SO2Cl2(g) + 16.1 kcal = SO2(g) + Cl2(g)If the TEMPERATURE on the equilibrium system is suddenly decreased: The reaction must:   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:   A. Increase.     B. Decrease.     C. Remain the same.

Consider the following exothermic reaction: 4 NH3 (g)   +   5 O2 (g)   ⇋⇋   4 NO (g)   +   6 H2O (l) How would the equilibrium shift if NH3 is added to the reaction mixture? Select one: a. The reaction would shift to the right. b. The reaction would shift to the left. c. The equilibrium would not be affected.

Choose the process that will not disturb the following equilibrium. Co(g) + H20(g) = CO2(g) + H2(g) A. Removing co O B. Increasing the temperature O C. Adding a catalyst D. Removing H2