Using Le Chatelier's Principle to predict the result of changing... Carbon disulfide and oxygen react to form carbon dioxide and sulfur dioxide, like this: CS₂(g) +30₂(g) → CO₂(g) +2SO₂(g) Suppose a mixture of CS₂, O₂, CO₂ and SO₂ has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some SO₂ is added. Some O₂ is removed. change in composition The pressure of CS₂ will The pressure of O₂ will The pressure of CS₂ will The pressure of CO₂ will ✓ ? ? ? go up. go down. not change. shift in equilibrium to the right to the left (none) to the right to the left O (none)

Using Le Chatelier's Principle to predict the result of changing... Carbon disulfide and oxygen react to form carbon dioxide and sulfur dioxide, like this: CS₂(g) +30₂(g) → CO₂(g) +2SO₂(g) Suppose a mixture of CS₂, O₂, CO₂ and SO₂ has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some SO₂ is added. Some O₂ is removed. change in composition The pressure of CS₂ will The pressure of O₂ will The pressure of CS₂ will The pressure of CO₂ will ✓ ? ? ? go up. go down. not change. shift in equilibrium to the right to the left (none) to the right to the left O (none)

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...

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Consider the following equilibrium: +2NOgCl2g 2NOClg = ΔG0−41.kJ Now suppose a reaction vessel is filled with 8.37atm of chlorine Cl2 and 4.00atm of nitrosyl chloride NOCl at 536.°C . Answer the following questions about this system: Under these conditions, will the pressure of Cl2 tend to rise or fall? rise fall Is it possible to reverse this tendency by adding NO ?In other words, if you said the pressure of Cl2 will tend to rise, can that be changed to a tendency to fall by adding NO ? Similarly, if you said the pressure of Cl2 will tend to fall, can that be changed to a tendency to rise by adding NO ? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it.Round your answer to 2 significant digits. atm
Consider the reaction N₂(g) + O₂(g) = 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.30, 0.30, and 0.025 atm, respectively, at 2200°C, what is Kp?
Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO2(g)+O2(9) 2 SO3(g) The reaction is exothermic. Suppose a mixture of SO,, O, and SO, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium O to the right O to the left: The temperature is raised. The pressure of 0, will O (none) to the right O to the left The temperature is lowered. The pressure of SO3 will 1? O (none) Submit A Continue MacBook Air O O O
Please provide proper explanation.
Using Le Chatelier's Principle to predict the result of changing... Ammonia and oxygen react to form nitrogen and water, like this: 4NH3 (g)+30₂ (g) 2N₂(g)+6H₂O(g) Suppose a mixture of NH3, O2, N₂ and H₂O has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some NH3 is added. Some H₂O is removed. change in composition The pressure of O₂ will The pressure of N₂ will The pressure of NH3 will ? ? ? shift in equilibrium to the right to the left O (none) to the right to the left
Consider the following equilibrium: N₂O4 (g) → 2NO₂ (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. O O rise fall yes no atm x10 X 5
Hydrogen chloride and oxygen react to form water and chlorine, like this: 4HCI(g)+O,(g) → 2H,0(g)+2Cl,(g) Suppose a mixture of HCI, 0,, H,0 and Cl, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. olo perturbation change in composition shift in equilibrium Ar O to the right The pressure of O, will ? to the left Some HCl is removed. The pressure of H20 will (none) to the right The pressure of HCl will ? Some H,0 is added. to the left The pressure of O, will (none)
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6) For the decomposition of ammonium nitrate at low temperature the equation is: NH,NO3 (s) → N20(g) + 2 H20(g) Assuming that Kc = 2.20 x 10ª at 25°C what is the pressure at equilibrium? What is the %3D pressure at 1000 K?
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Consider the following equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp = 3.67 x 101 at T = 75°C 2.50 atm of N2(g) and 2.50 atm of O2(g) are placed in a 3.00L flask and allowed to reach equilibrium. a) Write the Kp expression for this reaction. b) Determine the equilibrium partial pressures of each reactant and product. (BOX YOUR FINAL ANSWER.) c) Once the reaction is at equilibrium and the volume of the container is increased to 5.50 L, in which direction, if any, will the reaction proceed? Explain your answer.