The reaction CCl4--> C(graphite) + 2Cl2 has delta H= +95.7 kJ and delta S= +142.2 J/K at 25 degrees C. Calculate delta G.
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The reaction CCl4--> C(graphite) + 2Cl2 has delta H= +95.7 kJ and delta S= +142.2 J/K...
For the following reaction CCl4 (g) → C(s) + 2 Cl2 (g) Ho = +95.7 KJ; So = +142.2 J/K 1) What is Go for this reaction at 25 C? 2) What is the equilibrium constant for this reaction at 100 C? I need help with number 2) why would you not recalculate delta G for the reaction because its at a different temperature than 25C?
Consider the following reaction at 298 K. C(graphite)+2Cl2(g)⟶CCl4(l)ΔH∘=−139 kJC(graphite)+2Cl2(g)⟶CCl4(l)ΔH∘=−139 kJ Calculate the following quantities. Refer to the standard entropy values as needed. Consider the following reaction at 298 K. C(graphite) + 2Cl2(g) C014 (1) AH = -139 kJ Calculate the following quantities. Refer to the standard entropy values as needed. A$sys = 179.42 ASsurr = 466.44 A.Sunix =
A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta S° = -128.9 J/K The equilibrium constant for this reaction at 306.0 K is _______? Assume that Delta H° and DeltaS° are independent of temperature. B) For the reaction N2(g) + 3H2(g)---->2NH3(g) Delta H° = -92.2 kJ and Delta S° = -198.7 J/K The equilibrium constant for this reaction at 333.0 K is ___? Assume that Delta H° and Delta S° are independent of...
Consider the reaction at 298 K. C(graphite) + 2Cl2(8) — CCI (1) AH° = -139 kJ Calculate the quantities. ASsys = J/K S TOOLS A TOOLS x102 ASsurr = asyr = O JK J/K ASuniy = Asuniv = UK J/K
Consider the reaction at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ Calculate the quantities. Delta Ssys=_______ J/K Delata Ssurr =_______ J/K
a reaction has delta H = 100.0 kJ/mol and delta S = 250.0 J/mol K. Is the reaction spontaneous at room temperature? If no, at what temperature (in K and C) does this reaction become spontaneous?
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
A reaction has a delta H^0_Txn= -167.5 kJ/mol and delta S^0_Txn = 57.3 J/mo\ K. Calculate the equilibrium constant for the reaction. What is the difference between thermodynamic equilibrium constant and the apparent equilibrium constant?
Question 31 7.5 pts Determine AG ºrxn at 25°C using the following information CCI (9) → C (s, graphite) + 2Cl2 (9) AH°= +95.7 kJ; AS = +142.2 J/K +53.3k) 0 -348 kJ +440 kJ +28.4 kJ 0-58.3 kJ
Question 31 7.5 pts Determine AG rxn at 25°C using the following information CCI (9) → C (s, graphite) + 2Cl2 (9) AH°= +95.7 kJ; AS = +142.2 J/K +53.3 kJ 0 -348 kJ +440 kJ +28.4 kJ 0-58.3 kJ