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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 Kp for the reaction $$2N2(g)+O2(g) 2N2O(g) at 298.15 K and 1273 K....
Calculate the value of Kp for the reaction $$2N2(g)+O2(g) 2N2O(g) at 298.15 K and 1273 K. Thermodynamic data for N2O(g) are: ΔH°f = 82.05 kJ/mol; S° = 219.9 J/mol ·K; ΔG°f = 104.2 kJ/mol. Pt 1: 298.1K Pt 2: 1273 K
Use thermodynamic data to calculate the K_p for the reaction below at 298 K and 1300.0...
Use thermodynamic data to calculate the K_p for the reaction below at 298 K and 1300.0 K. 2 N_2(g) + O_2(s) 2 N_2 O(g)
Consider the reaction: FeO (s) + Fe (s) + O_2 (g) rightarrow Fe_2O_3 (s) Given the...
Consider the reaction: FeO (s) + Fe (s) + O_2 (g) rightarrow Fe_2O_3 (s) Given the following table of thermodynamic data, Substance Delta H_f degree S degree FeO (S) -271.9 kJ/mol 60.75 J/mol - K Fe (s) 0 27.15 O_2 (g) 0 205.0 Fe_2O_3 (S) -822.16 89.96 determine the temperature (in degree C) above which the reaction is nonspontaneous.
4.20 If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15...
4.20
If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. a. Calculate Delta H degree_ for ethanol at 298.15 K. b. Calculate Delta H degree_ of ethanol at 298.15 K. From the following data, calculate Delta H degree_ for the reaction CH_3COOH(g) rightarrow 2 H_2O(g) + 2 CO_2(g): Delta H degree _g (kJ mol^-1) CH_3COOH(l) + 2 O_2(g) rightarrow 2 H_2O(l) + 2 CO_2(g) -871.5 H_3O(l) rightarrow...
At 25 degree C, the following heats of reaction are known: 2CIF (g) + O_2 (g)...
At 25 degree C, the following heats of reaction are known: 2CIF (g) + O_2 (g) rightarrow Cl_2O (g)+ F_2O (g) Delta H_rxn^degree = 167.4 kJ/mol 2ClF_3 (g) +2O_2 (g) rightarrow Cl_2O (g) + 3F_2O (g) Delta H_rxn^degree = 341.4 kJ/mol 2F_2 (g) + O_2 (g) rightarrow 2F_2O (g) Delta H_rxn^degree = -43.4 kJ/mol At the same temperature, use Hess' law to calculate Delta H_rxn^degree for the following reaction: ClF (g) + F_2 (g) rightarrow ClF_3 (g)
For the gas-phase reaction 2SO_2 + O_2 doubleheadarrow 2SO_3, observed mole fractions for a certain equilibrium...
For the gas-phase reaction 2SO_2 + O_2 doubleheadarrow 2SO_3, observed mole fractions for a certain equilibrium mixture at 1000 K and 1767 torr are X_SO_2 = 0.310, X_O2= 0.190, and X_SO3= 0.500. Find K degree p and Delta G degree at 1000 K; assuming ideal gases, Find K_P at 1000 K. Find K degree C at 1000 K. K degree_P, and K degree_C have no units. Please enter them in 3 significant figures, e g. if the answer is 2.1,...
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 =...
Please show working! For the reaction SbCl_5(g) f SbCl_3(g) + Cl_2(g), Delta G degree _f (SbCl_5)...
Please show working!
For the reaction SbCl_5(g) f SbCl_3(g) + Cl_2(g), Delta G degree _f (SbCl_5) = -334.34 kJ/mol Delta G degree _f (SbCl_3) = -301.25 kJ/mol Delta H degree f (SbCl_5) = -394.34 kJ/mol Delta H degree _f (SbCl_3) = -313.80 kJ/mol Calculate the value of the equilibrium constant (K_P) for this reaction at 298 K.
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.
Consider the reaction 2CO(g) + 2NO(g) rightarrow 2CO_2(g) + N_2(g) for which Delta H degree =...
Consider the reaction 2CO(g) + 2NO(g) rightarrow 2CO_2(g) + N_2(g) for which Delta H degree = -746.6 kJ and Delta S degree = -198.0 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.514 moles of CO(g) react under standard conditions at 298.15 K. (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If...
Use thermodynamic data to calculate the K_p for the reaction below at 298 K and 1300.0 K. 2 N_2(g) + O_2(s) 2 N_2 O(g)
Consider the reaction: FeO (s) + Fe (s) + O_2 (g) rightarrow Fe_2O_3 (s) Given the following table of thermodynamic data, Substance Delta H_f degree S degree FeO (S) -271.9 kJ/mol 60.75 J/mol - K Fe (s) 0 27.15 O_2 (g) 0 205.0 Fe_2O_3 (S) -822.16 89.96 determine the temperature (in degree C) above which the reaction is nonspontaneous.
4.20
If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. a. Calculate Delta H degree_ for ethanol at 298.15 K. b. Calculate Delta H degree_ of ethanol at 298.15 K. From the following data, calculate Delta H degree_ for the reaction CH_3COOH(g) rightarrow 2 H_2O(g) + 2 CO_2(g): Delta H degree _g (kJ mol^-1) CH_3COOH(l) + 2 O_2(g) rightarrow 2 H_2O(l) + 2 CO_2(g) -871.5 H_3O(l) rightarrow...
At 25 degree C, the following heats of reaction are known: 2CIF (g) + O_2 (g) rightarrow Cl_2O (g)+ F_2O (g) Delta H_rxn^degree = 167.4 kJ/mol 2ClF_3 (g) +2O_2 (g) rightarrow Cl_2O (g) + 3F_2O (g) Delta H_rxn^degree = 341.4 kJ/mol 2F_2 (g) + O_2 (g) rightarrow 2F_2O (g) Delta H_rxn^degree = -43.4 kJ/mol At the same temperature, use Hess' law to calculate Delta H_rxn^degree for the following reaction: ClF (g) + F_2 (g) rightarrow ClF_3 (g)
For the gas-phase reaction 2SO_2 + O_2 doubleheadarrow 2SO_3, observed mole fractions for a certain equilibrium mixture at 1000 K and 1767 torr are X_SO_2 = 0.310, X_O2= 0.190, and X_SO3= 0.500. Find K degree p and Delta G degree at 1000 K; assuming ideal gases, Find K_P at 1000 K. Find K degree C at 1000 K. K degree_P, and K degree_C have no units. Please enter them in 3 significant figures, e g. if the answer is 2.1,...
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 =...
Please show working!
For the reaction SbCl_5(g) f SbCl_3(g) + Cl_2(g), Delta G degree _f (SbCl_5) = -334.34 kJ/mol Delta G degree _f (SbCl_3) = -301.25 kJ/mol Delta H degree f (SbCl_5) = -394.34 kJ/mol Delta H degree _f (SbCl_3) = -313.80 kJ/mol Calculate the value of the equilibrium constant (K_P) for this reaction at 298 K.
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.
Consider the reaction 2CO(g) + 2NO(g) rightarrow 2CO_2(g) + N_2(g) for which Delta H degree = -746.6 kJ and Delta S degree = -198.0 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.514 moles of CO(g) react under standard conditions at 298.15 K. (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If...
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