Part ADinitrogen tetroxide decomposes to form nitrogen dioxide according to the following reaction:2NO2 (g), Kp = 6.7 at 298 KN2O4 (g)2A reaction vessel contains 0.60 atm of N₂O4 and 2.0 atm NO2. Which statement is true of thereaction system?► View Available Hint(s)O The reaction system is at equilibrium.O The reaction system proceeds to the right (forming more product).O The reaction system proceeds to the left (forming more reactant).OIt is impossible to determine the future progress of the reaction based on the informationgiven.SubmitP PearsonInc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |

Part A Dinitrogen tetroxide decomposes to form nitrogen dioxide according to the following reaction: 2NO2(g), Kp = 6.7 at 298 K N₂O4 (g) = A reaction vessel contains 0.60 atm of N₂O4 and 2.0 atm NO₂. Which statement is true of the reaction system? ►View Available Hint(s) The reaction system is at equilibrium. The reaction system proceeds to the right (forming more product). The reaction system proceeds to the left (forming more reactant). It is impossible to determine the future progress of the reaction based on the information given. Submit P Pearson All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us

Part A Dinitrogen tetroxide decomposes to form nitrogen dioxide according to the following reaction: 2NO2(g), Kp = 6.7 at 298 K N₂O4 (g) = A reaction vessel contains 0.60 atm of N₂O4 and 2.0 atm NO₂. Which statement is true of the reaction system? ►View Available Hint(s) The reaction system is at equilibrium. The reaction system proceeds to the right (forming more product). The reaction system proceeds to the left (forming more reactant). It is impossible to determine the future progress of the reaction based on the information given. Submit P Pearson All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 94QAP: Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial...

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Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial pressures of I2(g), H2(g), and HI(g) for the system 2HI(g)H2(g)+I2(g) at 500°C if the initial partial pressures are all 0.200 atm.
Consider the following equilibrium: 2NO2g N2O4g = ΔG0−5.4kJ Now suppose a reaction vessel is filled with 8.33atm of dinitrogen tetroxide N2O4 at 294.°C . Answer the following questions about this system: Under these conditions, will the pressure of N2O4 tend to rise or fall? rise 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 ? yes no 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. atm
Natural gas is composed of 90% methane (CH4). As a heat source, methane is burned under the stream of O2. This reaction, namely combustion reaction, is given as follows :CH4(g) + 2O2(g) ↔ CO2(g) +2H2O(l)According to this reaction find out ΔAoreaction and ΔGoreaction at 298 K. So (CO2) = 213.8 J/mol.K ; So (H2O) = 70.0 J/mol.K ; So (CH4) = 183.6 J/mol.K ; So(O2) = 205.2 J/mol.K ; ΔHoreaction = -890 kJ/mol.Assume that all reactants and products behave as an ideal gase.
Consider the following equilibrium: 2NH3g +N2g3H2g = ΔG034.kJ Now suppose a reaction vessel is filled with 8.34atm of ammonia NH3 and 7.19atm of nitrogen N2 at 76.°C . Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? rise fall Is it possible to reverse this tendency by adding H2 ?In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2 ? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H2 ? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it.Round your answer to 2 significant digits. atm
Phosphorus pentachloride gas partially decomposes to phosphorus trichloride gas and chlorine gas. A 1.20 mol PCl5 is placed in a 1.00 L container at 200°C. At equilibrium 1.00 mol PCl5 remains. Calculate Kc and Kp at 200°C.
Consider the following reaction at equilibrium A + B ⇌ 2C and assume all are in the gas phase Kp =2.80E3 Calculate ΔGrxn for the reaction at 25 degrees C under standard conditions. Report your answer in Joules to three significant figures and do not use scientific notation.
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
Ammonium chloride is sometimes used as a flux in soldering because it decomposes on heating; NH4Cl (s) NH3 (g) + HCl (g) The HCl formed removed oxide films from metals to be soldered. In a certain equilibrium system at 400 ̊C, 22.6 g of NH4Cl is present; the partial pressures of NH3 and HCl are 2.5 atm and 4.5 atm, respectively. Calculate Kp at 400 ̊C.
Incomplete combustion of hydrocarbons produces the toxic gas Carbon monoxide can be eliminated by the reaction shown: CO + H2O ⇌ CO2 + H2 ΔH° = −41.0 kJ/mol and ΔS° = −42.3 J cal/(mol·K) at 25°C and 1 atm. What is ΔG° for this reaction? (What is ΔG if the gases have the following partial pressures: P(CO) = 1.3 atm, P(H2O) = 0.8 atm, P(CO2) = 2.0 atm, and P(H2) = 1.3 atm? What is ΔG if the temperature is increased to 150°C assuming no change in pressure?
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 3.00 L flask. The flask is found to contain 21.8 g of N₂O₄ and 2.65 g of NO₂ at 25°C. What are the values of Kc and Kp for this reaction? N₂O₄(g) ⇌ 2 NO₂(g) 1 2 NEXT Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms. Kc =
Consider the following equilibrium: 2NOClg +2NOgCl2g = ΔG041.kJ Now suppose a reaction vessel is filled with 9.13atm of nitrosyl chloride NOCl and 3.32atm of nitrogen monoxide NO at 934.°C . Answer the following questions about this system: Under these conditions, will the pressure of NO tend to rise or fall? rise fall Is it possible to reverse this tendency by adding Cl2 ?In other words, if you said the pressure of NO will tend to rise, can that be changed to a tendency to fall by adding Cl2 ? Similarly, if you said the pressure of NO will tend to fall, can that be changed to a tendency to rise by adding Cl2 ? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure of Cl2 needed to reverse it.Round your answer to 2 significant digits. atm
For the reaction: ½F2(g)F(g), a reaction mixture initially contains 1.5 atm of F2(g) and 1.5 atm of F(g) in their standard states. If Kp = 12 at this temperature, which statement is true? Q < K, and the reaction proceeds towards the products. Q > K, and the reaction proceeds towards the reactants. Q = K, and the reaction is at equilibrium. Q < K, and the reaction proceeds towards the reactants.