Consider the reaction: N2(g) + 3 F2(g) → 2 NF3(g) AH° = -249 kJ and AS° = -278 J/K at 25°C Calculate AG° and state whether the reaction is reactant favored or product favored at standard conditions. AG° = -166 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor products. None of these AG° = -166 kJ; the equilibrium composition should favor products.

Consider the reaction: N2(g) + 3 F2(g) → 2 NF3(g) AH° = -249 kJ and AS° = -278 J/K at 25°C Calculate AG° and state whether the reaction is reactant favored or product favored at standard conditions. AG° = -166 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor products. None of these AG° = -166 kJ; the equilibrium composition should favor products.

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

Initially 10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of nitrogen gas is found in the container. The number of moles of ammonia gas at equilibrium would be? 2NH3(g) + 94 kJ <=====> N2(g) + 3H2(g)
Consider the following chemical equation for which the enthalpy of reaction equals +26.9 kJ. 2 ICI(g) 12(g) + Cl2(g) At 25 °C, Kp = 5.0 x 10-6. If the temperature is increased to 35.0 °C, what changes (if any) will be observed? O a. Kp will remain unchanged. O b. Kp will increase. O c. [12] will decrease. O d. Kp will decrease. O e. [ICI] will increase.
Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.
Given the overall reaction from the previous problem: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) Using Le Chatelier’s principle, predict which direction the reaction will shift to reestablish equilibrium for each of the following changes: Calculate the enthalpy of reaction for this reaction using the standard thermodynamics values for the reactants and products. Is the reaction endothermic or exothermic? Now, use Le Chatelier’s principle again to determine the direction the equilibrium will shift if heat is added to the reaction. If 35 kPa of CO is mixed with 35 kPa of hydrogen in a 1.5 L container at 25°C, what is the theoretical yield of methane?
Identify the reactions that are exothermic. ) Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation... SHOW MORE V C(graphite)C(diamond) AH° = 2 kJ b. CaCO3 (s) CaO(s) + CO2(g) AH° = 178 kJ CuO(s) + H2 (g) → Cu(s) + H2 0(g) AH° = -85 kJ 2H2 (g) + 02(g) - 2H20(g) AH = -484 kJ 3H2 (g) + N2(g) 2NH3 (g) AH - 92 kJ Unanswered
The change in standard free energy (i.e. ΔG°) for a particular reaction has a value of −43.1 kJ/mol at a temperature of 16.1 ℃. Calculate the equilibrium constant for this reaction. R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation. Note: Your answer is assumed to be reduced to the highest power possible.
Given the following equation, N20(g) + NO28) → 3 NO(g) AG°rxn = -23.0 kJ Calculate AG° rxn for the following reaction. 3N20(g) + 3NO2(g) 9 NO(g) -23.0 kJ 69.0 kJ -69.0 kJ -7.67 kJ 23.0 kJ
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3 NO₂(g) + H₂O(1) – 2 HNO3 (1)+NO(g) -52.83 kJ/mol AGTxn Incorrect
Determine the AG° for the reaction of hydrogen and oxygen to form water. 2H2 (g) + O2 (g)→ 2H2O (g) AS°= -89.0 J/K AH°= -483.6 KJ
Which of the following statements about the storage of energy using chemical systems are correct? Mark all that are true. A. When energy is stored in a system where Q > K, energy is released from storage when the forward reaction occurs. B. Storing energy in a chemical system requires taking the system away from equilibrium. C. If AG° is negative, the forward reaction will always release energy and the reverse reaction will always store energy. D. The energy available by carrying out the forward reaction will change unless we take some additional action to hold Q constant.
6. Eqn 1: ZnS(s) Eqn 2: S(s) + O2(g) →SO2(g) Eqn 3: ZnS(s) + O2(g)→ Zn(s) + SO>(g) → Zn(s) + S(s) AG° = +198.3 kJ AG° =-300.1 kJ The decomposition of zinc sulfide (represented by Equation 1) can be accomplished by coupling the reaction to the combustion of sulfur (represented in Equation 2), which results in the overall reaction represented in Equation 3. a. Determine the free energy change for the reaction represented in Equation 3. b. Explain why the reactions represented in Equations 1 and 2 are suitable for coupling to produce a thermodynamically favorable process.
Consider the reaction. 2 Fe,O, 4 Fe + 30, AHn = +824.2 kJ The formation of 84.0 g of Fe results in the absorption of 3.10 x 102 kJ of heat. the absorption of 17300 kJ heat. the absorption of 1240 kJ of heat. the release of 1240 kJ of heat. the release of 3.10 x 10² kJ of heat. the release of 17300 kJ of heat. G Search or type URL