# College Chemistry

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The eqm. Constant for a reaction is 2.48 at 25°C. what is the value of ΔG° (kJ) at this temperature? (R=8.314 J/k mol)

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The eqm. Constant for a reaction is 2.48 at 25°C. what is the value of ΔG° (kJ) at this temperature?
2. ### College Chemistry

The eqm. Constant for a reaction is 2.48 at 25°C. what is the value of ΔG° (kJ) at this temperature?
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THE EQUILIBRIUM CONSTANT FOR A REACTION IS 2.48 AT 25 DEGREES CELSIUS. WHAT IS THE VALUE OF ΔG°(KJ)AT THIS TEMPERATURE?
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THE EQUILIBRIUM CONSTANT FOR A REACTION IS 2.48 AT 25 DEGREES CELSIUS. WHAT IS THE VALUE OF ΔG°(KJ)AT THIS TEMPERATURE?
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THE EQUILIBRIUM CONSTANT FOR A REACTION IS 2.48 AT 25 DEGREES CELSIUS. WHAT IS THE VALUE OF ΔG°(KJ)AT THIS TEMPERATURE?
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Can you check my calculations, please? It's for a lab we did in order to find the the enthalpy of formation of NH4Cl(s). My final answer was -299.4 kJ, while the theoretical, or actual, value is -314.4 kJ. It was the closest value
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I've figured out the Ea but I'm not sure how to find the kcal/mol The gas reaction N2O5 → 2NO2 + 1/2O2 follows the Arrhenius equation k = Ae(-Ea/RT) where R = 8.314 J K-1 mol-1 and 1 calorie = 4.184J. At the temperature T=273K, …
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In the following hypothetical reaction A + B → C + D, the equilibrium constant, Keq is less than 1.0 at 25°C and decreases by 35% on changing the temperature to 45°C. What must be true according to this information?

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