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From the following data: P_4(s) + 10Cl_2(g) rightarrow 4PCl_5A(s)...
Use the reactions provided below and their associated enthalpies to find delta_rH for the reaction PCl_3(l)...
Use the reactions provided below and their associated enthalpies to find delta_rH for the reaction PCl_3(l) + Cl_2(g) rightarrow PCl_5(s) at 25 degree C and 1 bar, (b) Calculate the corresponding enthalpy of reaction a 65 degree C if delta_r C_p, m = -50 J K^-1 mol^-1 (constant from 25-65 degree C). Does the reaction enthalpy increase or decrease with temperature? Given reactions (25 degree C, 1 bar): 2 P(s) + 3 Cl_2(g) rightarrow PCl_3(l) delta_rH = -640 kJ/mol Reaction...
Use Hess's Law to determine Delta H for the reaction 2 Al(s) + 3 Cl_2(g) rightarrow...
Use Hess's Law to determine Delta H for the reaction 2 Al(s) + 3 Cl_2(g) rightarrow 2 AlCl_3(s) given: 2 Al(s) + 6 HCl(aq) rightarrow 2 AlCl_3(aq) + 3 H_2(g) Delta H = -1049 kJ HCl(g) rightarrow HCl(aq) Delta H = -74.8 kJ H_2(g) + Cl_2(g) rightarrow 2 HCl(g) Delta H = -185 kJ AlCl_3(s) rightarrow AlCl_3(aq) Delta H = -323 kJ
Calculate the standard enthalpy change for the following reaction 2Al_2O_3(s) + 3C(s) rightarrow 4Al + 3CO_2(g)...
Calculate the standard enthalpy change for the following reaction 2Al_2O_3(s) + 3C(s) rightarrow 4Al + 3CO_2(g) given the following: delta H CO_2(g) = -393.5 kJ/mol delta H C(s) = 0 kJ/mol delta H Al = 10.79 kJ/mol delta H Al_2O_3(s) = -1675.7 kJ/mol
Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H =...
Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H = - 852 kJ What is Delta H when 0.100 mal of Al_2O_3 react with 0.250 mol of Fe? _____ kJ Using the data from Appendix G of the textbook, calculate Delta H for the combustion of 1.00 mole of C_2H_5OH(l). Note that (g) or (l) after the chemical formula denotes whether the compound is a gas or liquid. Some compounds have entries for both....
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?
At elevated temperatures, BrF_5 establishes the following equilibrium. 2BrF_5(g) Br_2(g) + 5F_2(g) The equilibrium concentrations of...
At elevated temperatures, BrF_5 establishes the following equilibrium. 2BrF_5(g) Br_2(g) + 5F_2(g) The equilibrium concentrations of the gases at 1500 K are 0.0064 mol/L for BrF_5, 0.0018 mol/L for Br_2, and 0.0090 mol/L for F_o. Calculate the value of K_r. The reaction of iron and water vapor results in an equilibrium 3Fe(s) + 4H_2O(g) Fe_3O_4(s) + 4H_2(g) and an equilibrium constant, K_c, of 4.6 at 850 degree C. What is the concentration of hydrogen present at equilibrium if the reaction...
I dont understand how to use hess's law to figure this out Given the following data:...
I dont understand how to use hess's law to figure this out
Given the following data: Fe_2 O_3 (s) + 3 CO(g) rightarrow 2 Fe(s) + 3 CO_2 (g) delta H = -23 kJ 3 Fe_2 O_3 (s) + CO(g) rightarrow 2 Fe_3 O_4 (s) + CO_2 (g) delta H = -39 kJ Fe_3 O_4 (s) + CO(g) rightarrow 3 FeO(s) + CO_2 (g) delta H = +18 kJ calculate delta H for the reaction FeO(s) + CO(g) rightarrow Fe(s)...
For the following reaction at 25.0 degree C, 2 C(s) + O_2(g) rightarrow 2 CO(g) calculate...
For the following reaction at 25.0 degree C, 2 C(s) + O_2(g) rightarrow 2 CO(g) calculate Delta S degree_univ given Delta S degree_sys = 179.1 J/K and Delta H degree_sys = -221.1 kJ.
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 =...
Consider the following reaction at 298 K: 2Al(s) + 3Cl_2 (g) rightarrow 2AlCl_3(s) delta H degree...
Consider the following reaction at 298 K: 2Al(s) + 3Cl_2 (g) rightarrow 2AlCl_3(s) delta H degree = -1408.4 kJ Calculate the following quantities. Find standard entropy values
Use the reactions provided below and their associated enthalpies to find delta_rH for the reaction PCl_3(l) + Cl_2(g) rightarrow PCl_5(s) at 25 degree C and 1 bar, (b) Calculate the corresponding enthalpy of reaction a 65 degree C if delta_r C_p, m = -50 J K^-1 mol^-1 (constant from 25-65 degree C). Does the reaction enthalpy increase or decrease with temperature? Given reactions (25 degree C, 1 bar): 2 P(s) + 3 Cl_2(g) rightarrow PCl_3(l) delta_rH = -640 kJ/mol Reaction...
Use Hess's Law to determine Delta H for the reaction 2 Al(s) + 3 Cl_2(g) rightarrow 2 AlCl_3(s) given: 2 Al(s) + 6 HCl(aq) rightarrow 2 AlCl_3(aq) + 3 H_2(g) Delta H = -1049 kJ HCl(g) rightarrow HCl(aq) Delta H = -74.8 kJ H_2(g) + Cl_2(g) rightarrow 2 HCl(g) Delta H = -185 kJ AlCl_3(s) rightarrow AlCl_3(aq) Delta H = -323 kJ
Calculate the standard enthalpy change for the following reaction 2Al_2O_3(s) + 3C(s) rightarrow 4Al + 3CO_2(g) given the following: delta H CO_2(g) = -393.5 kJ/mol delta H C(s) = 0 kJ/mol delta H Al = 10.79 kJ/mol delta H Al_2O_3(s) = -1675.7 kJ/mol
Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H = - 852 kJ What is Delta H when 0.100 mal of Al_2O_3 react with 0.250 mol of Fe? _____ kJ Using the data from Appendix G of the textbook, calculate Delta H for the combustion of 1.00 mole of C_2H_5OH(l). Note that (g) or (l) after the chemical formula denotes whether the compound is a gas or liquid. Some compounds have entries for both....
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?
At elevated temperatures, BrF_5 establishes the following equilibrium. 2BrF_5(g) Br_2(g) + 5F_2(g) The equilibrium concentrations of the gases at 1500 K are 0.0064 mol/L for BrF_5, 0.0018 mol/L for Br_2, and 0.0090 mol/L for F_o. Calculate the value of K_r. The reaction of iron and water vapor results in an equilibrium 3Fe(s) + 4H_2O(g) Fe_3O_4(s) + 4H_2(g) and an equilibrium constant, K_c, of 4.6 at 850 degree C. What is the concentration of hydrogen present at equilibrium if the reaction...
I dont understand how to use hess's law to figure this out
Given the following data: Fe_2 O_3 (s) + 3 CO(g) rightarrow 2 Fe(s) + 3 CO_2 (g) delta H = -23 kJ 3 Fe_2 O_3 (s) + CO(g) rightarrow 2 Fe_3 O_4 (s) + CO_2 (g) delta H = -39 kJ Fe_3 O_4 (s) + CO(g) rightarrow 3 FeO(s) + CO_2 (g) delta H = +18 kJ calculate delta H for the reaction FeO(s) + CO(g) rightarrow Fe(s)...
For the following reaction at 25.0 degree C, 2 C(s) + O_2(g) rightarrow 2 CO(g) calculate Delta S degree_univ given Delta S degree_sys = 179.1 J/K and Delta H degree_sys = -221.1 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 =...
Consider the following reaction at 298 K: 2Al(s) + 3Cl_2 (g) rightarrow 2AlCl_3(s) delta H degree = -1408.4 kJ Calculate the following quantities. Find standard entropy values
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