Ammonia and oxygen react to form nitrogen and water, like this: 4NH, (g)+30,(g) 2N,(g)+6H,O(g) do Suppose a mixture of NH2, O2, N, and H,0 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 Oto the right The pressure of NH3 will Some N, is added. O to the left The pressure of Oz will ? O (none) O to the right The pressure of O, will O to the left Some NH, is removed. The pressure of N2 will O (none) Submit Assignme Continue MacBook Air FI0 F8 吕口 D00 000 F4 F5 F3 F2 % 9

Ammonia and oxygen react to form nitrogen and water, like this: 4NH, (g)+30,(g) 2N,(g)+6H,O(g) do Suppose a mixture of NH2, O2, N, and H,0 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 Oto the right The pressure of NH3 will Some N, is added. O to the left The pressure of Oz will ? O (none) O to the right The pressure of O, will O to the left Some NH, is removed. The pressure of N2 will O (none) Submit Assignme Continue MacBook Air FI0 F8 吕口 D00 000 F4 F5 F3 F2 % 9

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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The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism:
For the gaseous reaction, 2 H2 + 2 NO ⟷ 2 H2O + N2, K at 120oC = 2.42. At a given moment, it is found that the concentrations of H2, NO, H2O and N2 are 1.1, 1.3, 0.78 and 2.2 M, respectively. Which of the following statements describes the situation? Group of answer choices Q = 1.2 so the reaction goes to the right Q = 1.2 so the reaction goes to the left Q = 0.65 so the reaction goes to the right Q = 0.65 so the reaction goes to the left The reaction is at equilibrium
Hydrogen and fluorine react to form hydrogen fluoride, like this: H,(9)+F,(9) → 2 HF(g) The reaction is exothermic. Suppose a mixture of H,, F, and HF 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 to the right to the left The temperature is raised. The pressure of H2 will ? (none) to the right The temperature is lowered. to the left The pressure of HF will ? O (none) ?
Acetylene and oxygen react to form carbon dioxide and water, like this: 2C,H,(g)+50,(g) → 4CO,(s)+2H,0(g) Suppose a mixture of C,H,, O,, CO, and H,O 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. alo perturbation change in composition shift in equilibrium O to the right The pressure of O, will to the left Some C,H, is added. The pressure of CO, will O (none) O to the right The pressure of C,H, will ? O to the left Some Co, is removed. The pressure of O2 will O (none) I Don't Know Submit O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center Accessibility DD F11 F12 80 F9 F10 F8 F7 F6 F5 F4 esc F2 F3 & #3 $ @
2. Assume that the reaction fort he formation of gaseous hydrogen fluoride (HF) from hydrogen and fluoride has an equilibrium constant of Kc = 1.15x10 at a certain temperature. H2(g) + F:(g) 2HF(g) In a particular experiment, 3.00 moles of each component were added to a 1.50 L flask. a) Calculate the reaction quotient, Qc, b) Calculate the equilibrium concentrations of all species.
The following equilibrium constants were determined at 1123K (picture). Calculate the equilibrium constant at 1123K for C(s)+CO2(g)+Cl2(g) 2COCl2(g). Explain how you got your answer.
The pressure-based equilibrium constant for the reaction shown below is Kp = 0.974 at 357 ℃. What is the value of Kc at this temperature? CH3OH(g) ⇌ CO(g) + 2 H2(g) R = 0.082058 L⋅atm/mol⋅K. Report your answer to THREE significant figures.
Consider the reaction: N,04(g)2NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K1 and K2, for the reactions below: N2(g) + 2 O2(g) =N,04(g) Kı 1/2 N2(g) + O2(g) =NO2(g) K2 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K,2 if the first equilibrium constant should be squared. K =
Hydrogen sulfide and oxygen react to form sulfur dioxide and water, like this: 2H₂S (g) + 30₂(g) → 2SO₂(g) + 2H₂O(g) Suppose a mixture of H₂S, O₂, SO2 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 SO₂ is added. Some H₂S is removed. change in composition The pressure of H₂S will The pressure of O₂ will The pressure of O₂ will The pressure of SO₂ will ? ? ? ? ↑ ↑ ↑ ↑ shift in equilibrium X O OOO to the right to the left (none) to the right to the left (none) Ś
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc= (_______) / (_______) = (______) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. N₂(g) + O₂(g) ⇌ 2 NO(g) Initial (M) Change (M) Equilibrium (M) Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴ Based on your ICE table and expression for Kc, solve for the…