For reactions carried out under standard-state conditions, the equation \( \Delta G = \Delta H - T \Delta S \) becomes\[ \Delta G^\circ = \Delta H^\circ - T \Delta S^\circ \]Assuming \( \Delta H^\circ \) and \( \Delta S^\circ \) are independent of temperature, one can derive the equation:\[ \ln \left( \frac{K_2}{K_1} \right) = \frac{\Delta H^\circ}{R} \left( \frac{T_2 - T_1}{T_1 T_2} \right) \]where \( K_1 \) and \( K_2 \) are the equilibrium constants at \( T_1 \) and \( T_2 \), respectively. Given that at 25.0°C, \( K_c \) is \( 4.63 \times 10^{-3} \) for the reaction\[ \text{N}_2\text{O}_4(\text{g}) \rightleftharpoons 2\text{NO}_2(\text{g}) \]\[ \Delta H^\circ = 58.0 \, \text{kJ/mol} \]calculate the equilibrium constant at 63.0°C.\[ K_c = \_\_\_\_\_ \]

The given relation is, lnK2K1=∆HoRT2-T1T1T2 Where, K1 and K2 are the equilibrium…

For reactions carried out under standard-state conditions, the equation AG= AH- TAS becomes AG =H - TAS.Assuming AH and AS equation: are independent of temperature, one can derive the K2 AH T2-T1 In- K1 R where K and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, K, is 4.63 x 103 for the reaction N204(g) 5 2NO2(g) AH = 58.0 kJ/mol calculate the equilibrium constant at 63.0°C. K =

For reactions carried out under standard-state conditions, the equation AG= AH- TAS becomes AG =H - TAS.Assuming AH and AS equation: are independent of temperature, one can derive the K2 AH T2-T1 In- K1 R where K and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, K, is 4.63 x 103 for the reaction N204(g) 5 2NO2(g) AH = 58.0 kJ/mol calculate the equilibrium constant at 63.0°C. K =

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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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 7.45 atm of nitrosyl chloride (NOCI) and 6.59 atm of chlorine (Cl₂) at 335. °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
3. Consider the following reaction: Co(g) + 2H2(g) S CH;OH(g); Kp = 2.26x10ª at 25 °C Calculate AG for the reaction at 25 °C for each of the following conditions: (a) standard conditions (b) at equilibrium (c) P (CH3OH) = 1.0 atm, P (CO) = P (H2) = 0.010 atm
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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 4.89 atm of ammonia (NH,) and 5.72 atm of nitrogen (N,) at 847. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding H,? In other words, if you said the pressure of NH, will tend to rise, can that 3 yes be changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of NH, will tend to fall, can that be changed to a tendency to 3 rise by adding H,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. 2. atm Round your answer to 2 significant digits.
Consider the following equilibrium: 2NH₂ (g)-N₂ (g) + 3H₂(g) AG-34. KJ Now suppose a reaction vessel is filled with 4.85 atm of ammonia (NH3) a system: Under these conditions, will the pressure of H, tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of H, will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of H₂ 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. and 2.40 atm of hydrogen (H₂) at 658. °C. Answer the following questions about this Ⓒrise O fall yes no atm 10 10 X S
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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=-108 kJ, and K. 77.5, at 600 K. CO(g) + C,(g) COCI,(g) When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish cquilibrium. O remain the same. It is already at cquilibrium. The concentration of CO will Submit Answer Retry Entire Group 1 more group attempt remaining
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ient/takeCovalentActivity.do?locator-assignment-take Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x102, at 1.15x10° K. 2S03(g) 2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value ofK. A. increases. B. decreases. C. remains the same. The value of Q. A. is greater than K.. B. is equal to K. C. is less than K. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of O, will: A. increase. B. decrease. C. remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Prev