Using reaction free energy to predict equilibrium composition elld Consider the following equilibrium: N2 (g) + 3H2 (g) = 2NH3 (g) AGº = -34. kJ Now suppose a reaction vessel is filled with 6.04 atm of nitrogen (N2) and 9.12 atm of ammonia (NH3) at 892. °C. Answer the following questions about this system: ? rise x10 fall Under these conditions, will the pressure of N2 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of N2 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of N₂ will tend to fall, can that be changed to a tendency to rise by adding H₂? 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. yes no ☐ atm ☑ ⑤ 000 18 Ar Bi

Using reaction free energy to predict equilibrium composition elld Consider the following equilibrium: N2 (g) + 3H2 (g) = 2NH3 (g) AGº = -34. kJ Now suppose a reaction vessel is filled with 6.04 atm of nitrogen (N2) and 9.12 atm of ammonia (NH3) at 892. °C. Answer the following questions about this system: ? rise x10 fall Under these conditions, will the pressure of N2 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of N2 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of N₂ will tend to fall, can that be changed to a tendency to rise by adding H₂? 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. yes no ☐ atm ☑ ⑤ 000 18 Ar Bi

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: 2NH, (g) – N, (g) + 3H, (g) AG° = 34. kJ Now suppose a reaction vessel is filled with 5.02 atm of ammonia (NH,) and 9.40 atm of nitrogen (N,) at 159. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N, tend to rise or fall? fall Is it possible to reverse this tendency adding H2? In other words, if you said the pressure of N, will tend to rise, can that be yes changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of N, will tend to fall, can that be changed to a tendency to rise by adding H2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, 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
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For the reaction below, what is the effect of raising the temperature? 4A(g) + B(g) 3C(g) AH = - 405 kJ Equilibrium shifts to the right; the reaction makes more products. O The reaction makes more of both products and reactants, so equilibrium is unaffected O Equilibrium re-establishes Equilibrium shifts to the left; the reaction makes more reactants.
At -8.64 °C the concentration equilibrium constant K = 7.7 for a certain reaction. Here are some facts about the reaction: -1 • The initial rate of the reaction is 5.3 mol·L¯¹·s¯¹. . If the reaction is run at constant pressure, 132. kJ/mol of heat are absorbed. • The constant pressure molar heat capacity C = 2.97 J'mol K¹. Yes. Using these facts, can you calculate K at 16. °C? x10 O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 16. °C will be bigger or smaller than K at -8.64 °C? C Yes, and K will be bigger. Yes, and K will be smaller. No.
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[Review Topics] [References) Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° =-10.4 kJ/mol, and K. = 55.6 , at 698 K. H2 (g) + I2 (g)=2 HI (g) When 0.26 moles of HI (g) are added to the equilibrium system at constant temperature: The value of K. The value of Q. v Ke The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of I, will Submit Answer Retry Entire Group 9 more group attempts remaining (Previ ins prt sc delete fg f10 f12
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