1. For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the direction of the product, the reactants, or does not change N, (g) + 0, (g) + heat 2NO (g) a. Increasing the temperature - b. Decreasing the volume of the container c. Adding a catalyst - d. Adding more N2 (g)

.Given the reaction at equilibrium: 2 A(g) + 3 B(g) <--> A2B3(g) + heat Which change will not affect the equilibrium concentrations of A(g), B(g) and A2B3(g)?     adding more A(g) adding a catalyst increasing the temperature increasing the pressure

Consider the following gas-phase equilibrium reaction: N2(g) + O2(g) 2NO(g); Kc = 4.10 x 10-4 at 2000 degrees C If 8.00 mol of NO is introduced into a 7.00 L container at 2000 degrees C, what is the concentration of NO when equilibrium is reached?

Pretend the following reaction is at equilibrium. How will the equilibrium shift if the volume is suddenly increased? N2(g) + 3H2(g) = 2NH3(g) A. shifts to products B. shifts to reactants C. no shifting

What will the concentration of PCl5 be when equilibrium is reestablished after addition of 1.31 g Cl2? PCl5(g) ⇆ PCl3(g) + Cl2(g) Original Equilibrium Mixture: 3.95 g PCl5 4.86 g PCl3 3.59 g Cl2 in a 1.00-L flask. [PCl5] = ? mol/L

Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed?  a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases

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

4 NH3(g) +5 O2(g) = 4 NO(g) + 6 H,0(g) AH =-904.4 kJ Consider the equilibrium system represented in the reaction above. Will the concentration of NO increase, decrease, or remain the same when the following experimental changes are made: a. NH, is added d. The volume of the container is reduced b. [H,O] is increased e. A catalyst is added c. O, is removed f. The temperature is increased

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