(i) (ii) (iii)

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17.101 The molecular scenes below depict the reaction Y at four different times, out of sequence, as it reaches equilibrium. Each sphere (Y is red and Z is green) represents 0.025 mol, and the volume is 0.40 L. (a) Which scene(s) represent(s) equilibrium? (b) List the scenes in the correct sequence. (c) Calculate K.. A

For the reaction N,0,(g) = 2NO,(g) Kc = 4.66 × 10-3 at 25°C . 2.50 g N,04 and 0.190 g NO, are introduced into a 2.00-L reaction vessel. After equilibrium is achieved, what is the concentration of NO,?

Consider the reaction: A B The equilibrium constant for this reaction is Kc = 10. Which of the following diagrams best represents this reaction at equilibrium? Hint: grey spheres = A green spheres = B Od O c Ob O a (a) (b) O (d)

Consider the reaction, 2AB2(g) = A2(g) + 2B2(g), Kc = 0.263 at 25°C. The reaction begins with an unknown concentration of AB2 in the reaction flask. At equilibrium, the concentration of AB2 is found to be 0.00545 M. a) Complete the ICEE table below, b) Write the equilibrium expression and equation for this reaction (pay close attention to coefficients!), c) Calculate the equilibrium concentration of both products, and d) Calculate the initial concentration of AB2. You should confirm that your equilibrium concentrations will give the correct equilibrium constant when plugged into the expression. ICEE table I C E 2 AB₂(g) A₂(g) + 2 B₂(g)

3. For the following reaction at equilibrium, 2BrNO(g) → 2NO(g) + Br2(g), what will happen if the volume of the container is decreased? (a) The reaction remains unchanged (b) The reaction will shift to the left (c) The reaction will shift to the right

Use the References to access important values if needed for this question. The equilibrium constant for the following reaction is 1.20×10-2 at 500K. PCI5(g) PCI3(g) + Cl½(g) If an equilibrium mixture of the three gases at 500K contains 3.57x10-2 M PCI,(g) and 2.23×102 M PCI3, what is the equilibrium concentration of Cl,? M Submit Answer Retry Entire Group 9 more group attempts remaining ed

(a) Determine whether the value of K of an equilibrium system will be affected or, unaffected by the following changes: Changes Value of K (affected or unaffected) (O Decreasing the temperature (1) Increasing the pressure of the system () Decreasing the concentration of reactant (b) The following graph represents the amount of CO formed at two different temperatures, T; and T. The reaction as shown below: C() + H,O(g) = co(g) + H(g) T = 385 K [co) T = 335 K time Based on the graph, determine whether the forward reaction is endothermic or exothermic. Predict if the concentration of H:0 gas increases, decreases or remains the same if the temperature is decreased to 298 K. Explain. A mixture of 0.350 M of H:0, 0.125 M of CO and 0.125 M of H: was prepared and allowed to reach equilibrium in a 1.00 L flask. The equilibrium concentration of H;0 is 0.182 M. Calculate the Ke of the reaction at constant temperature. (H)