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For the reaction C(s) + H_O(g) rightarrow CO(g) +...
Calculate S^0 of NH_3(g) for the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) using the...
Calculate S^0 of NH_3(g) for the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) using the following data: Delta G_f^0 of NH_3(g) = - 16 kJ/mol Delta H_f^0 of NH_3(g) = - 45.9 kJ/mol S^0 of H_2(g) = 131 J/mol. K S^0 of N_2(g) = 191.5 J/mol. K
For the reaction H_2(g) + Br_2 (g) rightarrow 2HBr(g) K_p = 3.6 times 10^4 at 1496...
For the reaction H_2(g) + Br_2 (g) rightarrow 2HBr(g) K_p = 3.6 times 10^4 at 1496 K. What is the value of K'_p for the following reaction at 1496 K? HBr(g) rightarrow 1/2 H_2(g) + 1/2 Br_2(g) K'_p =
Consider the following reaction: Ca(s) + 2 H_2O(l) rightarrow Ca(OH)_2(s) + H_2(g) Calculate the heat of...
Consider the following reaction: Ca(s) + 2 H_2O(l) rightarrow Ca(OH)_2(s) + H_2(g) Calculate the heat of reaction based on the following information: 2H_2(g) + O_2(g) rightarrow 2 H_2O(l) DeltaH = -572 kJ/mol CaO(s) + H_2O(l) rightarrow Ca(OH)_2(s) DeltaH = -64 kJ/mol CaCO_3(s) rightarrow CaO(s) + CO_2(g) DeltaH = +178.1 kJ/mol 2 Ca (s) + O_2(g) rightarrow 2 CaO(s) DeltaH = -1270 kJ/mol 13. Acetylene is used in blow torches, and bums according to the following equation: 2 C_2H_2(g) + 5...
How can I do the calculation Calculate the activation energy, E_a, for the reaction 2N_2O_5(g) rightarrow...
How can I do the calculation
Calculate the activation energy, E_a, for the reaction 2N_2O_5(g) rightarrow 4NO_2(g) + O_2(g) from the observed rate constants: k = 3.46 times 10^-5 s^-1 at 25 degree C and k = 1.5 times 10^-3 s^-1 at 55 degree C. a. 1437 kJ/mol b. 102 kJ/mol c. 0.101 kJ/mol d. 9.62 kJ/mol e. 1.04 kJ/mol
This is Thermodynamics in chemisty. Would you please teach both problems? For the reaction Fe O_(s)...
This is Thermodynamics in chemisty. Would you please teach both
problems?
For the reaction Fe O_(s) + H_2_(g) rightarrow Fe_(s) + H_2 O_(g) Delta H is 30.0 kJ/mole and Delta S is 24.0 J/mole-K. At what temperature will the reaction reach equilibrium? (A) 125 K (B) 298 K (C) 1250 K (D)2520 K (F) 760 K The Delta G degree for the ionization of HF is -20.5 kJ. Calculate the free energy change for ionization of hydrofluoric acid (K_a =...
The following reaction has an activation energy of 262 kJ/mol. C_4H_8(g) rightarrow 2C_2H_4(g) At 600.0 K...
The following reaction has an activation energy of 262 kJ/mol. C_4H_8(g) rightarrow 2C_2H_4(g) At 600.0 K the rate constant is 6.1 times 10^-8 s^-1. What is the value of the rate constant at 870.0 K?
Physical chemistry question For the reaction: creatine phosphate + H2O rightarrow creatine + P_i, delta G...
Physical chemistry question
For the reaction: creatine phosphate + H2O rightarrow creatine + P_i, delta G degree = 37.6 kJ at 310 K will the above reaction proceed forwards or backwards when the initial concentrations are: [creatine phosphate] = 1.2 times 10^-7 M [creatine] = 7.8 times 10^-1 M [P_i] = 9.2 times 10^-1 M
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.
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.
The following reaction has an activation energy of 262 kJ/mol. C4H8(g) rightarrow 2C2H4 (g). At 600.0...
The following reaction has an activation energy of 262 kJ/mol. C4H8(g) rightarrow 2C2H4 (g). At 600.0 K the rate constant is 6.1*10^-8 s^-1. What is the value of rate constant at 725.0K
Calculate S^0 of NH_3(g) for the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) using the following data: Delta G_f^0 of NH_3(g) = - 16 kJ/mol Delta H_f^0 of NH_3(g) = - 45.9 kJ/mol S^0 of H_2(g) = 131 J/mol. K S^0 of N_2(g) = 191.5 J/mol. K
For the reaction H_2(g) + Br_2 (g) rightarrow 2HBr(g) K_p = 3.6 times 10^4 at 1496 K. What is the value of K'_p for the following reaction at 1496 K? HBr(g) rightarrow 1/2 H_2(g) + 1/2 Br_2(g) K'_p =
Consider the following reaction: Ca(s) + 2 H_2O(l) rightarrow Ca(OH)_2(s) + H_2(g) Calculate the heat of reaction based on the following information: 2H_2(g) + O_2(g) rightarrow 2 H_2O(l) DeltaH = -572 kJ/mol CaO(s) + H_2O(l) rightarrow Ca(OH)_2(s) DeltaH = -64 kJ/mol CaCO_3(s) rightarrow CaO(s) + CO_2(g) DeltaH = +178.1 kJ/mol 2 Ca (s) + O_2(g) rightarrow 2 CaO(s) DeltaH = -1270 kJ/mol 13. Acetylene is used in blow torches, and bums according to the following equation: 2 C_2H_2(g) + 5...
How can I do the calculation
Calculate the activation energy, E_a, for the reaction 2N_2O_5(g) rightarrow 4NO_2(g) + O_2(g) from the observed rate constants: k = 3.46 times 10^-5 s^-1 at 25 degree C and k = 1.5 times 10^-3 s^-1 at 55 degree C. a. 1437 kJ/mol b. 102 kJ/mol c. 0.101 kJ/mol d. 9.62 kJ/mol e. 1.04 kJ/mol
This is Thermodynamics in chemisty. Would you please teach both
problems?
For the reaction Fe O_(s) + H_2_(g) rightarrow Fe_(s) + H_2 O_(g) Delta H is 30.0 kJ/mole and Delta S is 24.0 J/mole-K. At what temperature will the reaction reach equilibrium? (A) 125 K (B) 298 K (C) 1250 K (D)2520 K (F) 760 K The Delta G degree for the ionization of HF is -20.5 kJ. Calculate the free energy change for ionization of hydrofluoric acid (K_a =...
The following reaction has an activation energy of 262 kJ/mol. C_4H_8(g) rightarrow 2C_2H_4(g) At 600.0 K the rate constant is 6.1 times 10^-8 s^-1. What is the value of the rate constant at 870.0 K?
Physical chemistry question
For the reaction: creatine phosphate + H2O rightarrow creatine + P_i, delta G degree = 37.6 kJ at 310 K will the above reaction proceed forwards or backwards when the initial concentrations are: [creatine phosphate] = 1.2 times 10^-7 M [creatine] = 7.8 times 10^-1 M [P_i] = 9.2 times 10^-1 M
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.
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.
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