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- The standard Gibbs free energy for the reaction A + B → C is −(3.6x10^2) kJ at 298 K. What is the equilibrium constant for this reaction? Report your answer to 2 sig figs. Do not round in the middle of the calculation. how do I solve this please explain and also show how to type it in on desmos scientific calcEstimate reaction enthalpy and predict the sign of reaction entropy included attatchemnt of mecahnism and of original reactionEstimate the temperature at which the equilibrium constant for CuSO4 ⋅ 5 H2O(s) → CuSO4(s) + 5 H2O(g) becomes 1; assume pH2O = 1 bar.
- 2NO(g) + Br2(g) ↔ 2NOBr(g) , initial concentration of NO is 0.0655mol and 0.0328mol of Br2 . At equilibrium concentration of NOBr is 0.0389mol. Calculate Kp , Kc at 500C˚and vessel volume?What is the standard enthalpy of a reaction for w hichthe equilibrium constant is (a) doubled. (b) halved w hen thetemperature is increased by 10 Kat 298 K?For a C <->2D equilibrium reaction, if the enthalpy change at standard condition is 60 kJ/mol, if there is 20% decomposition at 1 bar and 1000⁰C, what is the K value at room temperature (25⁰C), the Gibbs energy change of the reaction under standard conditions, and the K value at 1200K?
- (a) For the ideal gas reaction A + B ↔ 2C + 2D, it is given that ∆Gθ500= 1250 cal mol-1. If 1.0 mol of A and 1.0 mol of B are placed in a vessel at 500 K and P is held fixed at 1200 torr, calculate the equilibrium amount of A, B, C, and D.Would it be reasonable to try to develop a catalyst for the reaction run at 298 K? Explain.What is the value of the equilibrium constant when ΔGorxn = 25 kJ·mol-1 and T=298 K?
- The standard Gibbs energy of formation of gaseous ozone at 25.0 ℃ ΔfGo, is162.3 kJ. mol-1, for standard state of 1 bar. The reaction is: 3O2 (g) ⇌ 2O3(g). Calculate the value of Kx at 2 bar.Consider the following general reaction: A(g) ⇌ B(g) Assuming that the ΔGo for this reaction is +50.2 J/mol, what is the equilibrium constant of this reaction at 420 K? (Please provide your answer to 3 significant figures.)Enthapy, ΔH = ΔE + PΔV is equal to q for reactions at constant pressure that a. involve only solids b. have gases as products, but not reagents c. have gases as reagents, but not products d. occur in aqueous solution