The equilibrium reaction below is endothermic.   N2O4(g) ⇋ 2 NO2(g)  Colorless     Brown gas                gas What is the color of gas generated when the following conditions are employed? a. The pressure is lowered.  b. The volume is increased.  c. The system is cooled.

Dinitrogen tetraoxide, a colorless gas, exists in equilibrium with nitrogen dioxide, a reddish brown gas. One way to represent this equilibrium is: N₂04(g) 2NO₂(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) NO₂(g) 1/2 N₂O4(g) K₁ 2) 1/2 N₂O4(9) NO₂(g) 3) 2NO₂(g) N₂O4(9) Drag and drop your selection from the following list to complete the answer: K¹/2 (1/K)¹/2 = = K₂ K3 = 1/K

Consider the exothermic reaction: A (g) + B (s) → 2X (g) @ 25 °C a. Propose a change in VOLUME so that the equilibrium position shifts towards the REACTANTS. b. Propose a change in TEMPERATURE so that the equilibrium position shifts towards the PRODUCTS. c. Propose a change in [A] so that the equilibrium position shifts towards the PRODUCTS.

Assuming the system is already at equilibrium, predict whether each of the following changes will cause the amount of CO2(g) to increase, decrease, or stay the same. 2 NaHCO3(s) <-> Na2CO3(s) + H2O(g) + CO2(g) H°= + 91.6 kJ/mol a. Increase the amount of NaHCO3(s)b. Increase the amount of Na2CO3(s)c. Increase the amount of H2O(g)d. Decrease the temperaturee. Addition of HCl (which catalyzes this reaction)f. Increase the volume of the reaction container