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6. Circle the value of ΔG when both products and reactants are in their standard states...
For the following reaction, all of the reactants and products are in their standard states/standard 1.0...
For the following reaction, all of the reactants and products are in their standard states/standard 1.0 M concentrations. Which of the following statements must be true? Zn(s) + SnBr2(aq) → ZnBr2(aq) + S (s) E-0.60 V OA AGº for the reaction as written is positive B. Zinc is undergoing reduction OC. None of the above OD. All of the above O E. The reaction would be product-favored as written
A particular gas-phase reaction has an equilibrium constant of 𝐾p=0.70 . A mixture is prepared where all the reactants and products are in their standard states. Which direction will the reaction proceed?
A particular gas-phase reaction has an equilibrium constant of 𝐾p=0.70Kp=0.70. A mixture is prepared where all the reactants and products are in their standard states.Which direction will the reaction proceed?) Q<K) Q>K) Q=K
2 NH3 (9)+ 3 o2(9) > 3 H20 (9) + NO2 (9) + NO (9) Use the data from this link:ThermodynamicData to calculate the following for the reaction above. (a)AG° at 298 K. kJ (b) Calculate the numerical v...
2 NH3 (9)+ 3 o2(9) > 3 H20 (9) + NO2 (9) + NO (9) Use the data from this link:ThermodynamicData to calculate the following for the reaction above. (a)AG° at 298 K. kJ (b) Calculate the numerical value of In K at 590 K (c) The temperature at which the reaction can be at equilibrium under standard conditions, if this is possible. If it is not possible, enter 0 (d) The ΔG at 590 K if all reactants in...
1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - &
1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - Keq <1 E° - ΔG° - Keq <1 E° + ΔG°+ Keq >1 E° + ΔG°- Keq >1 E° - ΔG° + Keq <1 2. What information can be obtained from the Figure below? The equivalence point occurs at pH = 7.0 but the pKa is not known from the graph. Both the pOH and the...
5. Consider a reaction starting with reactants and products in nonstandard state conditions, and a negative...
5. Consider a reaction starting with reactants and products in nonstandard state conditions, and a negative value of the nonstandard free energy change, AG. Which of the following best describes the redox reaction? A. Q=K and Ecell=0 B. Q<K and Ecell<0 c. Q<K and Ecell > 0 D. Q> K and Ecell <0 E. Q> K and Ecell > 6. The standard cell potential (Eºcell) of the reaction below is +1.08 V. What is the value of AGº for the...
When ΔG ̊=0, the system is at equilibrium and both the forward and reverse reaction are...
When ΔG ̊=0, the system is at equilibrium and both the forward
and reverse reaction are proceeding at equal rates. This is the
case during phase transitions. Consider the phase transition and
the data shown for BCl3 below. Calculate the boiling point (in ̊C)
for BCl3. BCl3(l) ⇄ BCl3(g) Hf ̊ (kJ/mole) S ̊ (J/mol∙K) BCl3(l)
-418 209 BCl3(g) -395 290
4. When AG°=0, the system is at equilibrium and both the forward and reverse reaction are proceeding at equal...
Equations AS-re/T, AS system= ES® (products) - ES (reactants); AS univ=AS sys+AS sur; AGⓇ-AH- AGG products...
Equations AS-re/T, AS system= ES® (products) - ES (reactants); AS univ=AS sys+AS sur; AGⓇ-AH- AGG products - Gractants; AGⓇ--RT In K TAS: Constants SJ/mol K): Na(s)=51.21, H20(1=69.95, NaOH(aq)-48.1, H2(g)=130.7 AHºr kJ/mol : Na(s)=0, H2O(I=-285.83, NaOH(aq)=-469.15, H2(g)=0 1) For the reaction: Na(s) + H2O(l) → NaOH(aq) + H2(g) at 298K a) Calculate AHºrn b) Calculate AS system c) Calculate AG® d) Explain why the reaction is favored by enthalpy, entropy favored, both or neither? e) Which direction does the equilibrium shift...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) +...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
The following reaction is exothermic. Which change will shift the equilibrium to the right? 2 SO2...
The following reaction is exothermic. Which change will shift the equilibrium to the right? 2 SO2 (g) + O2 (g) = 2 So, (9) o Adding So, Decreasing the volume of the reaction flask Removing O2 Heating the reaction QUESTION 11 A positive AGⓇ for a reaction implies The reaction is never spontaneous The products predominate at equilibrium The reaction is always spontaneous The reactants predominate at equilibrium ОО QUESTION 12 Which of the following is TRUE regarding AG and...
Q(18) NI(CO)49) - Ni(s) + 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium...
Q(18) NI(CO)49) - Ni(s) + 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends on the amount added Q(19) CO2 + H2 -CO + H2O Adding a catalyst to this reaction will cause the COD at equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it...
For the following reaction, all of the reactants and products are in their standard states/standard 1.0 M concentrations. Which of the following statements must be true? Zn(s) + SnBr2(aq) → ZnBr2(aq) + S (s) E-0.60 V OA AGº for the reaction as written is positive B. Zinc is undergoing reduction OC. None of the above OD. All of the above O E. The reaction would be product-favored as written
2 NH3 (9)+ 3 o2(9) > 3 H20 (9) + NO2 (9) + NO (9) Use the data from this link:ThermodynamicData to calculate the following for the reaction above. (a)AG° at 298 K. kJ (b) Calculate the numerical value of In K at 590 K (c) The temperature at which the reaction can be at equilibrium under standard conditions, if this is possible. If it is not possible, enter 0 (d) The ΔG at 590 K if all reactants in...
5. Consider a reaction starting with reactants and products in nonstandard state conditions, and a negative value of the nonstandard free energy change, AG. Which of the following best describes the redox reaction? A. Q=K and Ecell=0 B. Q<K and Ecell<0 c. Q<K and Ecell > 0 D. Q> K and Ecell <0 E. Q> K and Ecell > 6. The standard cell potential (Eºcell) of the reaction below is +1.08 V. What is the value of AGº for the...
When ΔG ̊=0, the system is at equilibrium and both the forward
and reverse reaction are proceeding at equal rates. This is the
case during phase transitions. Consider the phase transition and
the data shown for BCl3 below. Calculate the boiling point (in ̊C)
for BCl3. BCl3(l) ⇄ BCl3(g) Hf ̊ (kJ/mole) S ̊ (J/mol∙K) BCl3(l)
-418 209 BCl3(g) -395 290
4. When AG°=0, the system is at equilibrium and both the forward and reverse reaction are proceeding at equal...
Equations AS-re/T, AS system= ES® (products) - ES (reactants); AS univ=AS sys+AS sur; AGⓇ-AH- AGG products - Gractants; AGⓇ--RT In K TAS: Constants SJ/mol K): Na(s)=51.21, H20(1=69.95, NaOH(aq)-48.1, H2(g)=130.7 AHºr kJ/mol : Na(s)=0, H2O(I=-285.83, NaOH(aq)=-469.15, H2(g)=0 1) For the reaction: Na(s) + H2O(l) → NaOH(aq) + H2(g) at 298K a) Calculate AHºrn b) Calculate AS system c) Calculate AG® d) Explain why the reaction is favored by enthalpy, entropy favored, both or neither? e) Which direction does the equilibrium shift...
The following reaction is exothermic. Which change will shift the equilibrium to the right? 2 SO2 (g) + O2 (g) = 2 So, (9) o Adding So, Decreasing the volume of the reaction flask Removing O2 Heating the reaction QUESTION 11 A positive AGⓇ for a reaction implies The reaction is never spontaneous The products predominate at equilibrium The reaction is always spontaneous The reactants predominate at equilibrium ОО QUESTION 12 Which of the following is TRUE regarding AG and...
Q(18) NI(CO)49) - Ni(s) + 4 CO(g)Adding nickel (solid) to this reaction will cause the equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it depends on the amount added Q(19) CO2 + H2 -CO + H2O Adding a catalyst to this reaction will cause the COD at equilibrium to A) Shift toward the products B) Shift toward the reactants C) remain unchanged D) increase the temperature E) it...
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