Be sure to answer all parts.Nitrogen dioxide decomposes according to the reaction2 NO2(g) 2 NO(g) + O2(g)-13where Kp = 4.48 × 10¯¹³ at a certain temperature. If 0.30 atm of NO2 is added to a container andallowed to come to equilibrium, what are the equilibrium partial pressures of NO(g) and O2(g)?atm 02atm NO

Step 1: The ICE table for the given reaction can be constructed as 2 NO2 (g)2 NO (g)O2…

Answered: Be sure to answer all parts. Nitrogen…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 70QAP: For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of...

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Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?
Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g) At a certain temperature, the equilibrium partial pressures of SO2, Cl2, and SO2Cl2 are 1.88 atm, 0.84 atm, and 0.27 atm, respectively. (a) What is K at that temperature? (b) Enough Cl2 condenses to reduce its partial pressure to 0.68 atm. What are the partial pressures of all gases when equilibrium is reestablished?
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.
Gaseous acetic acid molecules have a certain tendency to form dimers. (A dimer is a molecules formed by the association of two identical, simpler molecules.) The equilibrium constant Kp at 25C for this reaction is 1.3 103. a If the initial pressure of CH3COOH monomer (the simpler molecule) is 7.5 103 atm, what are the pressures of monomer and dimer when the system comes to equilibrium? (The simpler quadratic equation is obtained by assuming that all of the acid molecules have dimerized and then some of it dissociates to monomer.) b Why do acetic acid molecules dimerize? What type of structure would you draw for the dimer? c As the temperature decreases, would you expect the percentage of dimer to increase or decrease? Why?
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
Consider the formation of HI(g) from H2(g) and I2(g). H2(g)+I2(g)2HI(g) For this reaction, K at 333C is 98, while K at 527C is 62.5. Find S for I2(g) at 527C.
The reaction PCl5(g) PCl3(g) + Cl2(g) was examined at 250 C. At equilibrium, [PCl5] = 4.2 105 mol/L, [PCl3] = 1.3 102 mol/L, and [Cl2] = 3.9 103 mol/L. Calculate Kc, for the reaction.
Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
Consider the formation of NO(g) from its elements. N2(g) + O2(g) 2 NO(g) (a) Calculate Kp at 25 C. Is the reaction product-favored at equilibrium at this temperature? (b) Assuming rH and rS are nearly constant with temperature, calculate rG at 700 C. Estimate Kp from the new value of rG at 700 C. Is the reaction product-favored at equilibrium at 700 C? (c) Using Kp at 700 C, calculate the equilibrium partial pressures of the three gases if you mix 1.00 bar each of N2 and O2.
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?

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