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DeltaH degree is +23 kJ mol^-1 of phosphine (PH_3) for the reaction Calculate Delta S degree...
Use deltaH and S to calculate DeltaG rxn... Use Delta H degree_f and S degree to...
Use deltaH and S to calculate DeltaG rxn...
Use Delta H degree_f and S degree to calculate Delta G degree rxn (Delta G degree sys) at 25 C for the reaction below: 4 KClO3 (s) rightarrow 3 KClO4 (s) + KCl (s) Delta H degree_f KClO3 = -397.7 kJ/mol; KClO4 = -432.8 kJ/mol; KCl = -436.7 kJ/mol S degree KClO3 = 143.1 kJ/mol; KClO4 = 151.0 kJ/mol; KCl = 82.6 kJ/mol
a) use the data given below and calculate the deltaH, delta S , delta G and...
a) use the data given below and calculate the deltaH, delta S , delta G and Kp at 25degrees celcius for the reaction 2NO(g) + O2 = 2 NO2(g) b) calculate the delta G for the reaction at 250 degrees celcius c) at what tempurature (degrees celcuis) is delta G equal to zero ? In what temperature range is this reaction product favoured? Compound NO - Delta Hf,kJ/mol =90.9 Delta S,J/mol.K =210.76 Compount O2 - Delta Hf,kJ/mol =0 Delta S,/j/mol.K=205.14...
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate...
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 certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50...
A certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50 J/K. Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to in the disorder of the system. Calculate Delta G degree for this reaction at 298 K. If this value is less than 1 kJ/mol then enter 0 in...
Using the values of Delta H and Delta S given, calculate Delta G for each of...
Using the values of Delta H and Delta S given, calculate Delta G for each of the reactions at 25 degree C and indicate whether the reactions are spontaneous or non-spontaneous. Explain. Delta H = 10.5 kJ/mol and Delta S = 30.0 J/K-mol Delta H = -10.5 kJ/mol and Delta S = 105. J/K-mol
a reaction has delta H = 100.0 kJ/mol and delta S = 250.0 J/mol K. Is...
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 the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol...
For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K-mol. Calculate deltaGdegree at 500degreeC. For the reaction H^2 (g) + S(s) right arrow H^2S(g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K mol. Use the deltaGdegree value calculated at 500degreeC. Calculate deltaG for this reaction at 1500degreeC if P(H^2, g) = P(H^2S, g) = 10.0 atm. Show all standard calculation.
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ...
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H degree =...
If, for a particular process, delta H = -214 kJ/mol and delta S = 450 J/mole...
If, for a particular process, delta H = -214 kJ/mol
and delta S = 450 J/mole K, the process will be. Please show work
too, I am trying hard to understand!
< > Options Due Monday, Nov 25, 11:59pm EST © Explain how spontaneity is affected by temperature Question If, for a particular process, AH = -214 and AS - 450k the process will be: Select the correct answer below: O spontaneous at any temperature O nonspontaneous at any temperature...
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5...
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5 J/K mol, DeltaG=130.3 KJ/mol, K=1.506x10^-23, Nonspontaneous until temp 1107.8 K or higher. What is the new concentration of CO2 at nonstandard temperature (1107.8k)?
Use deltaH and S to calculate DeltaG rxn...
Use Delta H degree_f and S degree to calculate Delta G degree rxn (Delta G degree sys) at 25 C for the reaction below: 4 KClO3 (s) rightarrow 3 KClO4 (s) + KCl (s) Delta H degree_f KClO3 = -397.7 kJ/mol; KClO4 = -432.8 kJ/mol; KCl = -436.7 kJ/mol S degree KClO3 = 143.1 kJ/mol; KClO4 = 151.0 kJ/mol; KCl = 82.6 kJ/mol
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 certain reaction has Delta H degree = -22.50 kJ and Delta S degree = -75.50 J/K. Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to in the disorder of the system. Calculate Delta G degree for this reaction at 298 K. If this value is less than 1 kJ/mol then enter 0 in...
Using the values of Delta H and Delta S given, calculate Delta G for each of the reactions at 25 degree C and indicate whether the reactions are spontaneous or non-spontaneous. Explain. Delta H = 10.5 kJ/mol and Delta S = 30.0 J/K-mol Delta H = -10.5 kJ/mol and Delta S = 105. J/K-mol
For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K-mol. Calculate deltaGdegree at 500degreeC. For the reaction H^2 (g) + S(s) right arrow H^2S(g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K mol. Use the deltaGdegree value calculated at 500degreeC. Calculate deltaG for this reaction at 1500degreeC if P(H^2, g) = P(H^2S, g) = 10.0 atm. Show all standard calculation.
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H degree =...
If, for a particular process, delta H = -214 kJ/mol
and delta S = 450 J/mole K, the process will be. Please show work
too, I am trying hard to understand!
< > Options Due Monday, Nov 25, 11:59pm EST © Explain how spontaneity is affected by temperature Question If, for a particular process, AH = -214 and AS - 450k the process will be: Select the correct answer below: O spontaneous at any temperature O nonspontaneous at any temperature...
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