1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) AH 298

1.1 1 (a) N₂(g) = + 180 kJ mol-¹ + O₂(g) (b) Increasing the pressure From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst 2NO (g) AH 298

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider three different equilibrium mixtures shown in representations [1]–[3]. (a) Which reaction has the largest equilibrium constant? (b) Which reaction has the smallest equilibrium constant?
9) Consider the following reaction: com nitrogen gas: N₂F4(g) = 2NF2(g) where AH = + 38.5 kJ/mol a) Predict the equilibrium change if the reaction mixture is heated at constant volume. b) Predict the equilibrium change is some N₂F4 is removed without changing the temperature or the pressure. c) Predict the equilibrium change if pressure is decreased at constant temperature. d) Predict the equilibrium change if a catalyst is added.
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%.
5. The Water Gas equilibrium, co (8) + H20 (g) = CO2 (g) + H2 (g) has a equilibrium position when the pressure of CO, H2O, CO2 and H2 are, respectively, 0.500 atm, 1.00 atm, 0.167 atm and 3.00 atm at 1100 K. (a) What is the value of Kp at 1100 K? (b) Is the system at 1100 K at an equilibrium position when the respective pressures are 1.00 atm, 2.00 atm, 0.334 atm and 6.00 atm? If not, then in which direction will the system shift?
SO₂ reacts with Cl₂ to form SO₂Cl₂. The equilibrium constant, Kp, for this reaction is 0.417 at 373 K. 4 SO₂(g) + Cl₂(g) =SO₂Cl₂(g) The standard enthalpy change for this reaction (AH°) is -67.2 kJ/mol. (a) Predict the effect on the production of SO₂Cl₂ when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 449 K. Kat 449 K =
In which direction is the equilibrium shifted with each of the following concentration changes for the given reaction: (a) increase [H,l; (b) increase [HCI]; (c) decrease [Cl,]; (d) decrease [HCI]? H2g) + Cl2(g) 2 2 HCI(g)
Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of SF2(g) is 1.1X10-4 atm and the partial pressure of F3SSF is 0.0484 atm. (a) Write a balanced equilibrium equation to represent this reaction. (b) Compute the equilibrium constant corresponding to the equation you wrote. (c) Some SF2 (at a partial pressure of 2.3X10-4 atm) is placed in a closed container at 298 K with some F3SSF (at a partial pressure of 0.0484 atm). Enough argon is added to raise the total pressure to 1.000 atm. Calculate the initial reaction quotient for the decomposition of F3SSF to SF2.
The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + 02 (g) 2 NO (g) K, = 0.0290 at 2400°C If the initial partíal pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). 0.112 atm (A) (B) 0.0290 atm (C) 0.688 atm (D) 0.0563 atm (E) 0.0611 atm
The following reaction takes place into a constant-volume flask at 427°C: CCL(g) = C(s) +2 C2(g) AH=132 kJ At 427°C, the equilibrium constant for the reaction given above is K. = 1.3×10-2. A flask is filled with 2.00 atm of CCl4 at 427°C. (a) What is the value of K for this reaction? (R=0.082 L.atm/mol.K) (b) What are the partial pressures of CClL, Ch and the total pressure at equilibrium? (c) How will the equilibrium pressure of CCl(g) change if the temperature is increased? (d) How will the equilibrium system respond if the volume of the flask is reduced?
Please answer ALL parts of the question and show your work. Consider this reaction: 2H2S(g) + 3O2(g) <-----> 2H2O(g) + 2SO2(g) H= -1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium is disturbed by (a) expanding the container (b) removing SO2 (c) rasing the temperature (d) water vapor is added
When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H2O(g) <--> CO2(g) + H2(g) +heat For each of the following changes at equilibrium, indicate whether the equilbrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) (d) adding more H2O(g) (e) decreasing the volume of the container
Consider the following system: 4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(l) AH = -1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N,(g)? (3) adding water? (4) expanding the container at constant pressure? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?