- Question 9 If You Observe The Following Reaction At Equilibrium It Is Possible To Tell Whether The Reaction Started Wit 1 (376.71 KiB) Viewed 51 times
- Question 9 If You Observe The Following Reaction At Equilibrium It Is Possible To Tell Whether The Reaction Started Wit 2 (388.02 KiB) Viewed 51 times
- Question 9 If You Observe The Following Reaction At Equilibrium It Is Possible To Tell Whether The Reaction Started Wit 3 (394.08 KiB) Viewed 51 times
- Question 9 If You Observe The Following Reaction At Equilibrium It Is Possible To Tell Whether The Reaction Started Wit 4 (465.29 KiB) Viewed 51 times
- Question 9 If You Observe The Following Reaction At Equilibrium It Is Possible To Tell Whether The Reaction Started Wit 5 (404.71 KiB) Viewed 51 times
- Question 9 If You Observe The Following Reaction At Equilibrium It Is Possible To Tell Whether The Reaction Started Wit 6 (202.7 KiB) Viewed 51 times
Sodium sulfate 10-hydrate, Na₂SO4-10H₂O, dehydrates according to the equation at 25° C. What is the pressure of water vapor at equilibrium -25 Na₂SO4-10H₂O(s) = Na₂SO₁(s) + 10H₂O(g) K₂= =4.08 x 10 with a mixture of Na₂SO 10H₂O and NaSO? B 3.64× 10-³ atm 6.39 × 10-13 atm 3.64 x 10-5 atm D4.08x10-25 atm Question 8 For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction must be insoluble. True B False 3 Points
Question 6 A Decreases A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO 3, from sulfur dioxide, SO 2, and oxyg O₂, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or pa pressure) of SO 3 is lower than it would be at lower temperatures. The balanced reaction equation is 2SO₂(g) + O₂(g) →2SO . What does the equilibrium constant for this reaction do as the temperature increases? B) Remains the same Resets Increases Question 7 4 10 OF 10 QUESTIONS REMAI - 3 Poi Sodium sulfate 10-hydrate, Na₂SO4 10H₂O, dehydrates according to the equation Na₂SO 10H₂O(s) = Na₂SO4(s) + 10H₂O(g) K₂=4.08 × 10-25 at 25° C. What is the pressure of water vapor at equilibriur JOU O NU CO 3 Poir
Question 5 10 OF 10 QUESTIONS REMAINING Question 6 3 Points hich of the following is the reaction quotient expression for the ionization of NH3 in water? The equilibrium constant for the action of NH3 with water is 1.76× 10-5. A Kb=[OH-]/[NH,] ®) Kb=[NH][NH,] KB=[NH] (D) Kb=[NH 4][OH-]NH, 3 Points necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO 3, from sulfur dioxide, SO₂, and oxygen, P2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. The balanced reaction equation is 2SO₂(g) +O₂(g) →2SO3(g)
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH₂(g) +H₂O(g) = 3H₂(g) +CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CHÂ, 0.126 M: H₂O, 0.242 M: CO, 0.126 M: H₂. 1.15 M. at a temperature of 760° C? B 6.28 -1.52 D1.52 6.28 Question 4 A Calculate the number of grams of HI that are at equilibrium with 1.25 mol of H₂ and 63.5 g of I at 448° C. H₂ L²= 2 2H1 K-50.2 at 448° C B 50 g 3.64× 10-5 g Ⓒ3.96 g 507 8 3 Points
Analysis of the gases in a sealed reaction vessel containing NH3, N₂ 2. and H₂ at equilibrium at 400° C established the concentration of N₂ to be 1.2 M and the concentration of H₂ to be 0.24 M 2 2 N₂(g) + 3H₂(g) + 2NH3(g) K = 0.50 at 400° C. What is the equilibrium molar concentration of NH3? A 0.0083 B 0.24 0.0091 B 0.091 Question 2 Under what conditions is N₂O3(g) → NO(g) + NO₂(g) spontaneous? At temperatures > 287°K At temperatures <273°K At temperatures <287°K 10 OF 10 QUESTIONS REMAINING At temperatures > 273°K 3 Points