Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NOCI (g) = 2NO (g) + Cl2 (g) AGº =41. kJ Now suppose a reaction vessel is filled with 7.85 atm of nitrosyl chloride (NOCI) and 5.15 atm of chlorine (C12) at 834. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of C₁₂ tend to rise or fall? ☐ x10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of C12 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of C₁₂ will tend to fall, can that be changed to a tendency to rise by adding 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. yes no atm ☑ 00. 18 Ar

Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NOCI (g) = 2NO (g) + Cl2 (g) AGº =41. kJ Now suppose a reaction vessel is filled with 7.85 atm of nitrosyl chloride (NOCI) and 5.15 atm of chlorine (C12) at 834. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of C₁₂ tend to rise or fall? ☐ x10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of C12 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of C₁₂ will tend to fall, can that be changed to a tendency to rise by adding 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. yes no atm ☑ 00. 18 Ar

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: 2NOC1 (g) 2NO(g) + Cl₂ (g) AG=41. KJ Now suppose a reaction vessel is filled with 3.76 atm of nitrosyl chloride (NOC1) and 6.26 atm of nitrogen monoxide (NO) at 1161. °C. Answer the following questions about this system: Under these conditions, will the pressure of NO tend to rise or fall? Is it possible to reverse this tendency by adding C1₂? 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 C1₂? Similarly, if you said the pressure of NO will tend to fall, can that be changed to a tendency to rise by adding Cl₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of C12 needed to reverse it. Round your answer to 2 significant digits. OO rise fall yes no atm x10 X Ś
Consider the following equilibrium: 2NH3 (g) = N2 (g)+ 3H, (g) AG = 34. kJ Now suppose a reaction vessel is filled with 7.65 atm of ammonia (NH,) and 0.884 atm of hydrogen (H,) at 600. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,? In other words, if you said the pressure of NH, will tend to rise, can that O yes be changed to a tendency to fall by adding N,? Similarly, if you said the O no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding N,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N, needed to reverse it. ||atm Round your answer to 2 significant digits.
Consider the following equilibrium: 2NO, (g) – N,04(g) AG = - 5.4 kJ Now suppose a reaction vessel is filled with 7.26 atm of dinitrogen tetroxide (N,O) at 95. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can that yes be changed to a tendency to fall by adding N0,? Similarly, if you said the no pressure of N,0, will tend to fall, can that be changed to a tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, needed to reverse it. atm Round your answer to 2 significant digits. O O
Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall 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. yes no ☐ atm X S
Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or 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? 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. оо rise fall yes no 0 atm x10 X Ś
Consider the following equilibrium: N,0, (g) = 2NO, (3) AG' = 5.4 kJ Now suppose a reaction vessel is filled with 0.496 atm of nitrogen dioxide (NO,) at 137. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NO, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,O,? In other words, if you said the pressure of NO, will tend to rise, can that O yes be changed to a tendency to fall by adding N,04? Similarly, if you said O no the pressure of NO, will tend to fall, can that be changed to a tendency to rise by adding N,0,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N,0, needed to reverse it. O atm Round your answer to 2 significant digits.
Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? 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 N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5
For the reaction 2 A(g) = B(g) + 3 C(g), we begin with only pure A(g) and the total pressure is 8.00 atm. We attain equilibrium. At equilibrium, the total pressure is 12.00 atm. What is the value of ∆G◦ for this reaction? The temperature is 25.0 ◦C throughout.
Consider the following equilibrium: 2NO(g) + Cl₂ (g) 2NOCI (g) AG=-41. kJ Now suppose a reaction vessel is filled with 1.55 atm of chlorine (C1₂). about this system: T Under these conditions, will the pressure of NOCI tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOC1 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding 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. and 4.77 atm of nitrosyl chloride (NOCI) at 683. °C. Answer the following questions Orise Ofall yes Ono atm O x10 X S
The steam reforming reaction of methane follows this chemical equation: CHA(g) + H50(g) - CO(g) + 3 H2(g) A H° = +193 kJ/mol At 298 K the reaction lies far to the reactant side with a very small equilibrium constant of 2.35 × 10-23. To obtain a significant amount of the desired hydrogen gas product, the reaction is operated at very high temperatures. What is the equilibrium constant at 1100 K?
Consider the following equilibrium: 2NO₂(g) → N₂O4 (g) AG = -5.4 kJ Now suppose a reaction vessel is filled with 0.202 atm of nitrogen dioxide (NO₂) at 504. °C. A Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O4? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O needed to reverse it. V Round your answer to 2 significant digits. Orise fall O yes no atm 0
Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 500. mL flask with 3.3 atm of sulfur dioxide gas and 3.2 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 2.6 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K₁ = 0 P x10 X Ś