Using reaction free energy to predict equilibrium compositionConsider the following equilibrium:2NO (g) +Cl₂ (g) = 2NOC1 (g)AGº = -41. kJNow suppose a reaction vessel is filled with 5.41 atm of chlorine (C12) and 7.54 atm of nitrosyl chloride (NOCI) at 582. °C. Answer thefollowing questions about this system:riseUnder these conditions, will the pressure of NOCI tend to rise or fall?x10fallIs it possible to reverse this tendency by adding NO?In other words, if you said the pressure of NOCI will tend to rise, can thatbe changed to a tendency to fall by adding NO? Similarly, if you said thepressure of NOCI will tend to fall, can that be changed to a tendency torise by adding NO?yesnoIf you said the tendency can be reversed in the second question, calculatethe minimum pressure of NO needed to reverse it.Round your answer to 2 significant digits.atm☑

Answered: Using reaction free energy to predict…

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: 2NO (g) + Cl, (g)=2NOC1 (g) AG° = - 41. kJ Now suppose a reaction vessel is filled with 7.88 atm of chlorine (Cl,) and 9.01 atm of nitrosyl chloride (NOCI) at 1114. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NOCI tend to rise or fall? Ox10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that yes be changed to a tendency to fall by adding NO? Similarly, if you said the no 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. atm Round your answer to 2 significant digits. O O
Consider the following equilibrium: N₂ (g) + 3H₂ (g) 2NH3 (g) AG=-34. KJ Now suppose a reaction vessel filled with 3.73 atm of nitrogen (N₂) and 1.60 atm of ammonia (NH3) at 493. °C. Answer the following questions about this system: Under these conditions, will the pressure of N, 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 significant digits. Ⓒrise fall O yes O no atm X S ? do Är
Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 2 NOCI(g) 2 NO(g) + Cl₂ (g) Round your answer to 2 significant digits.
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
Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant x at 25.0 °c for the following reaction. N₂(g) + 3H₂(g) 2 NH3(g) Round your answer to 2 significant digits. K = 1 0 x10 X
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 reaction at 298 K. 2 so2(g) + 02(9) → 2 so3(g) An equilibrium mixture contains 0,(g) and So, (g) at partial pressures of 0.49 atm and 2.7 atm, respectively. Using data from the Thermodynamic Data table, determine the equilibrium partial pressure of So, in the mixture. 7.2e12 X atm
At 13.7 °C the concentration equilibrium constant K = 2.0 × 10 for a certain reaction. Here are some facts about the reaction: • C The constant pressure molar heat capacity C₁ = 2.49 J-mol K. •If the reaction is run at constant pressure, 147. kJ/mol of heat are released. •If the reaction is run at constant pressure, the volume increases by 13.%. ○ Yes. Using these facts, can you calculate K, at 3.8 °C? x10 No. If you said yes, then enter your answer at right. Round it to 2 significant digits. n If you said no, can you at least decide whether Kat 3.8 °C will be bigger or smaller than K at -13.7 °C? Yes, and K will be bigger. Yes, and K will be smaller. No. x
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
For a certain chemical reaction, the standard Gibbs free energy of reaction at 30.0 °C is -61.4 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 x10 S
Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. C(s) + 2Cl₂(g) → CC14 (g) Round your answer to 2 significant digits. K = 0 10 X Ś
A2(g) + 3B2(g) -> 2AB3(g) where the ΔGorxn is -140 kJ and equilibrium constant at standard conditions is 3.5x1024. a) If we place 0.100 atm of AB3, 0.050 atm of B2, and 0.500 atm of A2 in a container at 25oC, which direction will the reaction go (if any) to reach equilibrium? b) What is the value of ΔGrxn assuming the temperature is maintained at 25oC?

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