Consider the following equilibrium process at 686. °C: CO₂(g) + H₂(g) co(g) + H₂O(g) The equilibrium concentrations of t

Post by **answerhappygod** » Thu Jun 30, 2022 6:23 pm

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 1 (26.96 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 2 (47.35 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 3 (28.49 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 4 (20.62 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 5 (12.7 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 6 (20.86 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 7 (22.82 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 8 (19.9 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 9 (7.96 KiB) Viewed 128 times

: Consider The Following Equilibrium Process At 686 C Co G H G Co G H O G The Equilibrium Concentrations Of T 10 (11.94 KiB) Viewed 128 times

Consider the following equilibrium process at 686. °C: CO₂(g) + H₂(g) co(g) + H₂O(g) The equilibrium concentrations of the reacting species are [CO] -0.0540 M. [H₂]-0.0420 M. [CO₂]-0.0840 M, and [H₂0] -0.0450 M Part 1 of 5 Calculate K for the reaction at 686. °C. Be sure your answer has the correct number of significant digits. Part 2 of 5 X If we add CO₂ to increase its concentration to 0.440 M, what will the concentrations of all the gases be when equilibrium is reestablished? Be sure your answer has the correct number of significant digits.
Part 3 of 5 Be sure your answer has the correct number of significant digits. [¹₂]-M Part 4 of 5 0x10 Part 5 of 5 X Be sure your answer has the correct number of significant digits. [co]-M = X Ś O x10 S Be sure your answer has the correct number of significant digits. [H₂O]-M
Consider the following equilibrium system: PCI, (g) + Cl₂(g) PCI, (g) Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case. Part 1 of 3 Cl₂ gas is removed from the system. Select the single best answer. O The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) Part 2 of 3 PCI, gas is added to the system. Select the single best answer. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) X
Part 3 of 3 PC13 gas is added to the system. Select the single best answer. The equilibrium will not change. O The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.)
Consider the following equilibrium system: A B AH-0.0 kJ mol Predict the change in the equilibrium constant K, that would occur if the temperature of the reacting system was raised. Select the single best answer. There is no change. K increases. K decreases.
Consider the reaction: kJ 250₂(g) + O₂(g) = 250, (g) AH--198.2 mol How would the concentrations of SO₂, O₂, and SO, at equilibrium change we were to increase the temperature? Select the single best answer for each part. Part 1 of 3 [s0₂]: There is no change. The concentration increases. The concentration decreases. Part 2 of 31 [0₂]: There is no change. The concentration increases. The concentration decreases.
[so,]: O The concentration decreases. The concentration increases. There is no change. X S
Pure NOCI gas was heated at 235 "C in a 1.50 L container. At equilibrium the total pressure was 1.14 atm and the NOCI pressure was 0.70 atm. The equilibrium process involving NOCI, NO, and Cl, is represented by the following equation: 2NOCI(g) 2NO(g) + Cl₂ (g) Part 1 of 2 Calculate the partial pressure of NO and Cl, in the system. Be sure each of your answer entries has the correct number of significant digits. PNO Pa, Part 2 of 2 atm Calculate the equilibrium constant Kp. Be sure your answer has the correct number of significant digits.
When heated, ammonium carbamate decomposes as follows: NH,CO,NH,(s)= 2NH,(g) + CO, (g) At a certain temperature the equilibrium pressure of the system is 0.718 atm. Calculate the K, for the reaction. Be sure your answer has the correct number of significant digits.
The formation of SO, from SO₂ and O₂ is an intermediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. The equilibrium constant, Kp. for the reaction 2SO₂(g) + O₂(g) 250, (g) is 0.13 at 803 °C. In one experiment, 2.00 mol SO, and 2.00 mol O₂ were initially present in a flask. What must the total pressure at equilibrium be in order to have a 61.0% yield of SO,? Be sure your answer has the correct number of significant digits.