1) Calculate ΔG (in kJ) at 298 K for some solid ZnF2, 0.067 M Zn2+ and...
1) Calculate ΔG (in kJ) at 298 K for some solid ZnF2,
0.067 M Zn2+ and 0.070 M F-(aq).
Hint given in feedback.
2) Endothermic reaction; decrease in
entropy:
Calculate the equilibrium constant at 24 K for a reaction with
ΔHrxno = 10 kJ and
ΔSrxno = -100 J/K. (Don't round unil the end.
Using the exponent enlarges any round-off error.)
Homework Answers
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1) Calculate ΔG (in kJ) at 298 K for some solid ZnF2, 0.067 M Zn2+ and...
Please help with these 1. Calculate ΔG (in kJ) at 298 K for some solid ZnF2,...
Please help with these 1. Calculate ΔG (in kJ) at 298 K for some solid ZnF2, 0.082 M Zn2+ and 0.039 M F-(aq). 2.Calculate the equilibrium constant at 45 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round unil the end. Using the exponent enlarges any round-off error. Calculate the equilibrium constant at 136 K for the thermodynamic data in the previous question. ( Problem 2)
1-Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ and...
1-Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round unil the end. Using the exponent enlarges any round-off error.) 2-Calculate the equilibrium constant at 103 K for the thermodynamic data in the previous question. Notice that Keq is larger at the larger temperature for an endothermic reaction.
Incorrect = 10 kJ and Calculate the equilibrium constant at 36 K for a reaction with...
Incorrect = 10 kJ and Calculate the equilibrium constant at 36 K for a reaction with AH ASrxn° = 100 J/K. Mark 0.00 out of 1.00 P Flag question Answer: 2.00e-16 Question 25 Not answered Calculate the equilibrium constant at 106 K for the thermodynamic data in the previous question Marked out of 1.00 Notice that Keg is dramatically larger for a larger temperature when there is a substantial positive increase in entropy, P Flag question Answer: Question 28 Assume...
1) Calculate the equilibrium constant at 138 K for the thermodynamic data in the previous question....
1) Calculate the equilibrium constant at 138 K for the thermodynamic data in the previous question. Notice that Keq is larger at the larger temperature for an endothermic reaction. 2) Endothermic reaction; increase in entropy Calculate the equilibrium constant at 40 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = 100 J/K.
Calculate ΔG° (kJ/mole) at 298 K forthe reaction below:2H2S(g) + 3O2(g) ⇋2H2O(g) +...
Calculate ΔG° (kJ/mole) at 298 K for the reaction below:2H2S(g) + 3O2(g) ⇋2H2O(g) + 2SO2(g)K=6.32×1010Enter a number to 2 decimal places.
Calculate the ΔG°rxn at 298 K using the following information. 2 HNO3(aq) + NO(g) → 3...
Calculate the ΔG°rxn at 298 K using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0
Use the following data to calculate the value of ΔG°rxn at 298 K for the reaction...
Use the following data to calculate the value of ΔG°rxn at 298 K for the reaction described by the given chemical equation. Include the units. Compound S°f (J/molK) DH°f (kJ/mol) CO (g) 197.7 –110.5 H2 (g) 130.7 0 CH4 (g) 186.3 –74.6 H2O (g) 188.8 –241.8 CO (g) + 3H2 (g) → CH4 (g) + H2O (g) I got -141.9 KJ/mol, but i think the units are wrong and I don't know why.
1.) Calculate ΔHºrxn ΔSsurr and ΔSºrxn to determine if the reaction is spontaneous at 298 K ΔHºf...
1.) Calculate ΔHºrxn ΔSsurr and ΔSºrxn to determine if the reaction is spontaneous at 298 K ΔHºf : PCl3(g) = -287 kj/mol ΔSºf : PCl3(g) = -3112 J/mol *K ΔSºf : P4(s) = 41.1 J/mol*K ΔSºf : Cl2(g)= 2230 J/mol *K P4(s) +6Cl2(g) ------> 4PCl3(g) 2.) Calculate ΔGºrxn from enthalpy and entropy values at 298 K 4NH3 (g) +5O2(g) -----> 4 NO(g) +6H2O(g) ΔHºf : NO(g) = 90.29 kj/mol ΔHºf: H2O(g) = -241.826 kJ/mol ΔHºf: NH3(g) = -45.9 kJ/mol ΔSºf : NO(g)...
Part 1.) A certain reaction has Ho = -26.10 kJ and So = 15.60 J/K. (a)...
Part 1.)
A certain reaction has Ho = -26.10 kJ and So = 15.60 J/K.
(a) Is this reaction exothermic, endothermic or isothermic
(neither)?
This reaction is ---Select--- exothermic endothermic or
isothermic .
(b) Does this reaction lead to a decrease, an increase, or no
change in the degree of disorder in the system?
This reaction leads to ---Select--- a decrease, an
increase, or no change in the disorder of the system.
(c) Calculate Go for this reaction at 298 K. If...
Given the information A+B⟶2D. ΔH∘=−794.8 kJ ΔS∘=377.0 J/K C⟶D. ΔH∘=449.0 kJΔS∘=−192.0 J/K calculate ΔG∘ at 298...
Given the information A+B⟶2D. ΔH∘=−794.8 kJ ΔS∘=377.0 J/K C⟶D. ΔH∘=449.0 kJΔS∘=−192.0 J/K calculate ΔG∘ at 298 K for the reaction A+B⟶2C
Incorrect = 10 kJ and Calculate the equilibrium constant at 36 K for a reaction with AH ASrxn° = 100 J/K. Mark 0.00 out of 1.00 P Flag question Answer: 2.00e-16 Question 25 Not answered Calculate the equilibrium constant at 106 K for the thermodynamic data in the previous question Marked out of 1.00 Notice that Keg is dramatically larger for a larger temperature when there is a substantial positive increase in entropy, P Flag question Answer: Question 28 Assume...
Part 1.)
A certain reaction has Ho = -26.10 kJ and So = 15.60 J/K.
(a) Is this reaction exothermic, endothermic or isothermic
(neither)?
This reaction is ---Select--- exothermic endothermic or
isothermic .
(b) Does this reaction lead to a decrease, an increase, or no
change in the degree of disorder in the system?
This reaction leads to ---Select--- a decrease, an
increase, or no change in the disorder of the system.
(c) Calculate Go for this reaction at 298 K. If...
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