### Calculating $ \Delta G^\circ $ from Equilibrium ConstantsTo determine the standard Gibbs free energy change ($ \Delta G^\circ $) for a reaction, we can use the equilibrium constant ($ K_p $) at a given temperature. The table below provides the necessary data to perform these calculations for several reactions:| Reaction | Temperature (°C) | $ K_p $ value ||----------------------------------------------|------------------|------------------|| $ \text{N}_2 (g) + \text{O}_2 (g) \rightarrow 2\text{NO} (g) $ | 2000 | $ 4.1 \times 10^{-4} $ || $ \text{H}_2 (g) + \text{I}_2 (g) \rightarrow 2\text{HI} (g) $ | 400 | 50.0 || $ \text{CO}_2 (g) + \text{H}_2 (g) \rightarrow \text{CO} (g) + \text{H}_2\text{O} (g) $ | 980 | 1.67 || $ \text{CaCO}_3 (s) \rightarrow \text{CaO} (s) + \text{CO}_2 (g) $ | 900 | 1.04 |### Explanation of Data- **Reaction**: The balanced chemical equation for each reaction.- **Temperature (°C)**: The temperature at which the equilibrium constant $ K_p $ is measured.- **$ K_p $ value**: The equilibrium constant for the reaction at the given temperature.### Calculation of $ \Delta G^\circ $The relationship between $ \Delta G^\circ $ and $ K_p $ is given by the equation:\[ \Delta G^\circ = -RT \ln (K_p) \]where:- $ R $ is the universal gas constant (8.314 J/(mol·K)).- $ T $ is the temperature in Kelvin (K).#### Steps to Calculate $ \Delta G^\circ $:1. **Convert Temperature to Kelvin**: \[ T(K) = T(°C) + 273.15 \]2. **Calculate \( \Delta

Answer: Relation between equilibrium constant and standard Gibbs free energy change is shown below:…

Calculate AG°for each of the following reactions from the equilibrium constant at the temperature given. Reaction Temperature (°C) N₂ (g) + O₂ (g) → 2NO (g) 2000 H₂(g) + 1₂ (g) →→→ 2HI (g) 400 CO₂ (g) + H₂ (g) → CO (g) + H₂O (g) 980 CaCO3 (s) → CaO (s) + CO₂ (g) 900 Kp value 4.1 x 10-4 50.0 1.67 1.04

Calculate AG°for each of the following reactions from the equilibrium constant at the temperature given. Reaction Temperature (°C) N₂ (g) + O₂ (g) → 2NO (g) 2000 H₂(g) + 1₂ (g) →→→ 2HI (g) 400 CO₂ (g) + H₂ (g) → CO (g) + H₂O (g) 980 CaCO3 (s) → CaO (s) + CO₂ (g) 900 Kp value 4.1 x 10-4 50.0 1.67 1.04

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...

See similar textbooks

Similar questions

Industrially, methanol is synthesized using the reaction Cog) + 2 H2(g) + CH;OH(g) Calculate the equilibrium constant at 298 K. AGP CO(g) = -137.2 kJ/mol; AGP H: (g)= 0; AGP CH:OH(g) = -162 kJ/mol
The equilibrium constant for the following reaction is 20.9 at 907 °C. 2 SO2(g) + O2(g) 2 SO3(g) K= 20.9 at 907 °C Calculate the equilibrium constant for the following reactions at 907 °C. (a) 2 SO3(g) 2 SO2(g) + 02(g) K= (b) SO3(g) SO (g) + 1/2 O2(g) K=
Calculate AGO at 605 K for H₂O(g) + 1/2 02(g) → H₂O₂(g) using the following data: AGO = H₂(g) +O₂(g) → H₂O₂(g) K = 8.9 × 10³6 at 605 K 2H₂(g) + O₂(g) → 2H₂O(g) K = 2.0 x 106 at 605 K kJ/mol
4
8.B A certain reaction has an equilibrium constant of K = 8.3×10$ at 25°C with a temperature-independent standard enthalpy of reaction of 34.2 kJ/mol. (a) What is the equilibrium constant at 37°C? (b) Use Le Chatelier's principle to defend your answer.
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
Carbon monoxide reacts with water according to the following equilibrium reaction: CO (g) H2O (g) CO2 (g) + H2 (g) For this reaction, K = 0.810 at a temperature of 1000.°C. Calculate the value of AG for this reaction at 1000.ºC. %3D
Calculate AGO at 600. K for using the following data: AGO = H₂O(g) + 1/2O₂(g) → H₂O2(g) H₂(g) + O₂(g) → H₂O2(g) K = 1.8 × 10³7 at 600. K 2H2(g) + O₂(g) → 2H₂O(g) K = 2.3 × 106 at 600. K kJ/mol
8. Given: 2 HI (g) H2 (g) + 12 (g) AH < 0 This reaction is placed in a closed vessel and allowed to reach equilibrium. If H2 is removed, would the vessel feel cold or warm? Explain.
The equilibrium constant for the following reaction is 67.6 at 232 °C. PCI 3(g) + Cl₂(g) PCI5(g) K = 67.6 at 232 °C Calculate the equilibrium constant for the following reactions at 232 °C. (a) PCI5(g) PCl3(g) + Cl₂(g) K= (b) 2 PCI5(g) 2 PCI3(g) + 2 Cl₂(g) K=
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
If a chemical reaction has AG°298 -29.4 kJ, what is the equilibrium constant Keg at 298 K? O 7.0 x 10-6 O 1.4 x 105 O 7.4 x 1011 O 1.4 x 10-12 Ο 11.9