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For the reaction SbCl_5(g) f SbCl_3(g) + Cl_2(g), Delta G degree _f (SbCl_5)...
For the reaction 2 HBr(g) + Cl_2(g) rightarrow 2 HCl(g) + Br_2(g) a. Write the equilibrium...
For the reaction 2 HBr(g) + Cl_2(g) rightarrow 2 HCl(g) + Br_2(g) a. Write the equilibrium constant expression for the reaction. b. Using the following G degree values, calculate Delta G degree for the reaction. HBr(g) = -53.22 kJ/mol HCl(g) = -95.27 kJ/mol Cl_2(g) = 0 kJ/mol Br_2(g) = 3.14 kJ/mol c. Calculate the equilibrium constant K_eq be at 298 K. d. Does this equilibrium lie more with reactants or products?
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...
25 Select True or False: For the reaction SbC15(9) — SbC13(g) + Cl2(g). AG f (SbC15)...
25 Select True or False: For the reaction SbC15(9) — SbC13(g) + Cl2(g). AG f (SbC15) = -334,34 kJ/mol AG°(SbC13) = -301.25 kJ/mol AHf (SbC15) = -394.34 kJ/mol AH°F (SbC13) = -313.80 kJ/mol This reaction proceeds spontaneously at 298 K and 1 atm pressure. True or False True False
For the reaction SbCl5(g) ? SbCl3(g) + Cl2(g),? ?
For the reaction SbCl5(g)? SbCl3(g) + Cl2(g),? ?(SbCl5) = -334.34 kJ/mol?(SbCl3) = -301.25 kJ/mol?(SbCl5) = -394.34 kJ/mol?(SbCl3) = -313.80 kJ/mol?Will this reaction proceed spontaneously at 298 K and 1 atm pressure?Can you please explain me how you got the answer? It is not making any sense to me
For the aqueous reaction the standard change in Gibbs free energy is Delta G degree =...
For the aqueous reaction the standard change in Gibbs free energy is Delta G degree = 7.53 kJ/mol. Calculate Delta G for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00400 M. The constant R = 8.3145 J/(K middot mol) Delta G =
Calculate the value of K, at 298 K, for each value of delta G degree. delta...
Calculate the value of K, at 298 K, for each value of delta G degree. delta G degree = 7.5 kJ/mol delta G degree = -9.0 kJ/mol
Calculate the value of K_p for the reaction 2N_2(g) + O_2(g) reversible 2N_2 O(g) at 298.15...
Calculate the value of K_p for the reaction 2N_2(g) + O_2(g) reversible 2N_2 O(g) at 298.15 K and 1173 K. Thermodynamic data for N_2 O(g) are: delta H degree_t = 82.05 kJ/mol; S degree = 219.9 J/mol middot K; delta G degree f = 104.2 kJ/mol. 298.15 K Did you consider the stoichiometry of the balanced equation for the reaction? Did you check your signs and units? Would you expect K_p at 1173 K to be greater than or less...
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at...
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at 298 K. Delta G degree (NO_2(g)) = 51.84 kJ/mol, Delta G degree (N_2 O_4 (g)) = 98.28 kJ/mol. Calculate Delta G at 298 K if the partial pressures of NO_2 and N_2O_4 are 0.37 atm and 1.62 atm, respectively. Express your answer using one significant figure.
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.
Given the following table, calculate F degree and Delta G degree for the reaction: Sn^4 +...
Given the following table, calculate F degree and Delta G degree for the reaction: Sn^4 + 2 - 2 Cl^-, S_n^2- g_2 Cl_2
For the reaction 2 HBr(g) + Cl_2(g) rightarrow 2 HCl(g) + Br_2(g) a. Write the equilibrium constant expression for the reaction. b. Using the following G degree values, calculate Delta G degree for the reaction. HBr(g) = -53.22 kJ/mol HCl(g) = -95.27 kJ/mol Cl_2(g) = 0 kJ/mol Br_2(g) = 3.14 kJ/mol c. Calculate the equilibrium constant K_eq be at 298 K. d. Does this equilibrium lie more with reactants or products?
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...
25 Select True or False: For the reaction SbC15(9) — SbC13(g) + Cl2(g). AG f (SbC15) = -334,34 kJ/mol AG°(SbC13) = -301.25 kJ/mol AHf (SbC15) = -394.34 kJ/mol AH°F (SbC13) = -313.80 kJ/mol This reaction proceeds spontaneously at 298 K and 1 atm pressure. True or False True False
For the aqueous reaction the standard change in Gibbs free energy is Delta G degree = 7.53 kJ/mol. Calculate Delta G for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00400 M. The constant R = 8.3145 J/(K middot mol) Delta G =
Calculate the value of K, at 298 K, for each value of delta G degree. delta G degree = 7.5 kJ/mol delta G degree = -9.0 kJ/mol
Calculate the value of K_p for the reaction 2N_2(g) + O_2(g) reversible 2N_2 O(g) at 298.15 K and 1173 K. Thermodynamic data for N_2 O(g) are: delta H degree_t = 82.05 kJ/mol; S degree = 219.9 J/mol middot K; delta G degree f = 104.2 kJ/mol. 298.15 K Did you consider the stoichiometry of the balanced equation for the reaction? Did you check your signs and units? Would you expect K_p at 1173 K to be greater than or less...
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at 298 K. Delta G degree (NO_2(g)) = 51.84 kJ/mol, Delta G degree (N_2 O_4 (g)) = 98.28 kJ/mol. Calculate Delta G at 298 K if the partial pressures of NO_2 and N_2O_4 are 0.37 atm and 1.62 atm, respectively. Express your answer using one significant figure.
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.
Given the following table, calculate F degree and Delta G degree for the reaction: Sn^4 + 2 - 2 Cl^-, S_n^2- g_2 Cl_2
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