A certain reaction has a ΔG value of 13.8 kJ/mol. What is the value of the equilibrium constant (K) for this reaction when the temperature is 295 K?
What is the value of K at 305 K when ∆Go = -4.75 kJ/mol?
Consider a process with ∆H = 37.6 kJ and ∆S = 99.5 J/K. At what temperature will this process be at equilibrium?
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A certain reaction has a ΔG value of 13.8 kJ/mol. What is the value of the...
A certain reaction has a ΔG value of 13.8 kJ/mol. What is the value of the equilibrium constant (K) for this reaction when the temperature is 295 K?
Consider these hypothetical chemical reactions: A⇌B,ΔG= 13.7 kJ/mol B⇌C,ΔG= -27.2 kJ/mol C⇌D,ΔG= 6.20 kJ/mol What is the free energy, ΔG, for the overall reaction, A⇌D? Express your answer with the appropriate units. ΔG = Firefly luciferase is the enzyme that allows fireflies to illuminate their abdomens. Because this light generation is an ATP-requiring reaction, firefly luciferase can be used to test for the presence of ATP. In this way, luciferase can test for the presence of life. The coupled reactions...
A reaction has an equilibrium constant of Kp=0.061 at 27 ∘C. Part A Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 6.98 kJ 0.839 kJ -6.98 kJ 0.628 kJ Part B Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K 298 K 158.7 K 6.762 × 103 K This reaction is nonspontaneous at all...
A certain reaction has an activation energy of 48.97 kJ/mol. At what Kelvin temperature will the reaction proceed 6.50 times faster than it did at 295 K?
The ΔG°\' of the reaction is -6.220 kJ ·mol–1. Calculate the equilibrium constant for the reaction. (Assume a temperature of 25° C.)
The ΔG°\' of the reaction is -6.220 kJ ·mol–1. Calculate the equilibrium constant for the reaction. (Assume a temperature of 25° C.)
A certain reaction has ΔH°= -19.5 kJ/mol and ΔS°= +42.7 J/mol K a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ΔG° for the reaction at 298K. d) Is the reaction spontaneous at 298 K under standard conditions?
For a particular reaction at 172.4 °C, Δ?=−269.73 kJ/mol ΔG=−269.73 kJ/mol, and Δ?=970.33 J/(mol⋅K) Calculate ΔG for this reaction at 14.3 °C.
1. 1) luciferin+O2 ⇌ oxyluciferin+light 2) ATP⇌AMP+PPi ΔG∘=−31.6 kJ/mol If the overall ΔG∘ of the coupled reaction is -1.21 kJ/mol , what is the equilibrium constant, K, of the first reaction at 11∘C? Round your answer to 3 significant figures. 2. When methanol (CH3OH) is combusted, such as when in a gasoline blend, the following reaction occurs: 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g) Based on the standard free energies of formation given, what is the standard free energy change for this reaction? Report the answer...
Part 1.) A certain reaction has Ho = -26.10 kJ and So = 15.60 J/K. (a) Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is ---Select--- exothermic endothermic or isothermic . (b) Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to ---Select--- a decrease, an increase, or no change in the disorder of the system. (c) Calculate Go for this reaction at 298 K. If...