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Question 7 0.5 pts Determine the sign of ASsur and ASsys for the following chemical reaction...
Calculate the LaTeX: \Delta Δ G°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) LaTeX:...
Calculate the LaTeX: \Delta Δ G°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) LaTeX: \longrightarrow ⟶ 7 N2(g) + 12 H2O(l) LaTeX: \Delta Δ G°rxn = ? LaTeX: \Delta Δ G°f (kJ/mol) –73.5 149.3 –237.1
3. (3 points) Hydrazine (N2H4) can react with oxyger in the following chemical reaction: NaH.(1 +0:0) - N2(g) + 2H20 (1...
3. (3 points) Hydrazine (N2H4) can react with oxyger in the following chemical reaction: NaH.(1 +0:0) - N2(g) + 2H20 (1) Calculate AH, for the reaction above, given the following data: 2NH3(g) + 3N20(g) - 4260) + 3H2000 AH,º=-1010. kJ/mol N20(g) + 3H2(g) → N2H (1) + H2O(1 AH-=-317 k!/inol 2NH3(g) + 40:09) - NzH4O + H20(1 AH,"=-143 kJ/mol H2(g) +4202(9) - H20(1) AH"=-286 kJ/mol
7. Consider the following reaction: H,(8)+CO,(8)=1,0(g)+CO(g) The value of the equilibrium constant K, for the reaction...
7. Consider the following reaction: H,(8)+CO,(8)=1,0(g)+CO(g) The value of the equilibrium constant K, for the reaction is 0.534 at 700°C. What is the value of K, for this reaction at 298 K? (5 points) (AH; (H20) = -241.8, AH;(CO) = -110.5, AH;(CO2) = -393.5 kJ/mol)
Question 29 (9 points) Consider the following reaction: 3C(s) + 4H2(g) → C3H8(8); AH° =-104.7 kJ;...
Question 29 (9 points) Consider the following reaction: 3C(s) + 4H2(g) → C3H8(8); AH° =-104.7 kJ; ASP = -287.4J/K at 298 K 1). What is AGⓇ for this reaction? 2). What is the equilibrium constant at 400.0 K for this reaction?
(2) (24 pts) A fuel cell produces electricity via a combustion reaction. A DMFC is a...
(2) (24 pts) A fuel cell produces electricity via a combustion reaction. A DMFC is a proton-exchange fuel cell that uses methanol CH3OH) as the fuel, which reacts with molecular oxygen to produce carbon dioxide and water. (a) (4 pts) Write the balanced combustion reaction for this methanol fuel cell. (b) (4 pts) Write the balanced half-reactions occurring at the cathode and anode of this fuel cell (assume standard acidic conditions) (e) (4 pts) Evaluate AGº (kJ) and AE° (V)...
7 Consider the following reaction at 298 K: NH3(g) +HCI(g)NH4CI(s) Using the thermochemical data at 298 K given below (a) Determine the AH for the reaction. (2 marks) (b) Determine the AG for the...
7 Consider the following reaction at 298 K: NH3(g) +HCI(g)NH4CI(s) Using the thermochemical data at 298 K given below (a) Determine the AH for the reaction. (2 marks) (b) Determine the AG for the reaction and comment on its value. (3 marks) (c) Determine the maximum work done available in the reaction. (3 marks) An equilibrium mixture, consisting of 0.5 atm of NHy(), 0.5 atm of HCKg) and excessive of NH Cl(s), is enclosed in a container at 298 K...
Question 23 10 pts The entropy change for the reaction ( ASºrxn) shown below is -121.8...
Question 23 10 pts The entropy change for the reaction ( ASºrxn) shown below is -121.8 J/K. Calculate AS°surr, AS°univ and AGºrxn at 298 K. N2(g) + 2O2(g) + 2NO2(g) AH°rxn = 66.4 kJ • (a) AS surr = [Select ] • (b) AS°univ = [Select ] • (c) AGºrxn = [Select ]
no. 3 COL LUPIC. 3. (20 pts) Use the following thermodynamic data (reported at 298 K...
no. 3
COL LUPIC. 3. (20 pts) Use the following thermodynamic data (reported at 298 K and 1 bar) to determine: Substance 4/Hº (kJ/mol) S. (I/K-mol) 4,6° (kJ/mol) N2H4(1) 50.53 121.21 149.4 159.4 N2H4(g) 95.4 Wap 238.9 205.14 191. 610 O2(g) 0 0 N2(g) H2O(1) -237.2 69.91 -285.83 SpA (3a) (5 pts) The molar enthalpy of vaporization of hydrazine N, H. (36) (5 pts) Whether liquid hydrazine vaporizes at 25°C and 1 bar? Hint: Calculate the free energy of vaporization...
The standard enthalpy change for the following reaction is -415 kJ at 298 K. Zn(s) + Ch(g) → ZnCl2() AH° = -415 k...
The standard enthalpy change for the following reaction is -415 kJ at 298 K. Zn(s) + Ch(g) → ZnCl2() AH° = -415 kJ What is the standard enthalpy change for the reaction at 298 K? ZnCl(s) — Zn(s) + Cl2(g) The standard enthalpy change for the following reaction is -50.6 kJ at 298 K. N2H40 - N2(g) + 2 H2(g) AH° = -50.6 kJ What is the standard enthalpy change for this reaction at 298 K? N2(g) + 2 H2(g)...
4) Calculate the ΔGrxn using the following information. 4 HNO3(g)+5N2H40)- 7 N2(8) +12 H200) -133.9 AH。f...
4) Calculate the ΔGrxn using the following information. 4 HNO3(g)+5N2H40)- 7 N2(8) +12 H200) -133.9 AH。f (kJ/mol) s°C/mol K) 50.6 -285.8 266.9 121.2 191.6 70.0 A. Determine the enthalpy change 1° for the reaction at 298 K B. Determine aSsurr for the re C. Determine aSsvs for the reaction. D.Find the entropy change of the universe. E. Determine △G"for this reaction. Will this reaction be spontaneous? E. Determine the equilibrium constant Kp at 298K.
3. (3 points) Hydrazine (N2H4) can react with oxyger in the following chemical reaction: NaH.(1 +0:0) - N2(g) + 2H20 (1) Calculate AH, for the reaction above, given the following data: 2NH3(g) + 3N20(g) - 4260) + 3H2000 AH,º=-1010. kJ/mol N20(g) + 3H2(g) → N2H (1) + H2O(1 AH-=-317 k!/inol 2NH3(g) + 40:09) - NzH4O + H20(1 AH,"=-143 kJ/mol H2(g) +4202(9) - H20(1) AH"=-286 kJ/mol
7. Consider the following reaction: H,(8)+CO,(8)=1,0(g)+CO(g) The value of the equilibrium constant K, for the reaction is 0.534 at 700°C. What is the value of K, for this reaction at 298 K? (5 points) (AH; (H20) = -241.8, AH;(CO) = -110.5, AH;(CO2) = -393.5 kJ/mol)
Question 29 (9 points) Consider the following reaction: 3C(s) + 4H2(g) → C3H8(8); AH° =-104.7 kJ; ASP = -287.4J/K at 298 K 1). What is AGⓇ for this reaction? 2). What is the equilibrium constant at 400.0 K for this reaction?
(2) (24 pts) A fuel cell produces electricity via a combustion reaction. A DMFC is a proton-exchange fuel cell that uses methanol CH3OH) as the fuel, which reacts with molecular oxygen to produce carbon dioxide and water. (a) (4 pts) Write the balanced combustion reaction for this methanol fuel cell. (b) (4 pts) Write the balanced half-reactions occurring at the cathode and anode of this fuel cell (assume standard acidic conditions) (e) (4 pts) Evaluate AGº (kJ) and AE° (V)...
7 Consider the following reaction at 298 K: NH3(g) +HCI(g)NH4CI(s) Using the thermochemical data at 298 K given below (a) Determine the AH for the reaction. (2 marks) (b) Determine the AG for the reaction and comment on its value. (3 marks) (c) Determine the maximum work done available in the reaction. (3 marks) An equilibrium mixture, consisting of 0.5 atm of NHy(), 0.5 atm of HCKg) and excessive of NH Cl(s), is enclosed in a container at 298 K...
Question 23 10 pts The entropy change for the reaction ( ASºrxn) shown below is -121.8 J/K. Calculate AS°surr, AS°univ and AGºrxn at 298 K. N2(g) + 2O2(g) + 2NO2(g) AH°rxn = 66.4 kJ • (a) AS surr = [Select ] • (b) AS°univ = [Select ] • (c) AGºrxn = [Select ]
no. 3
COL LUPIC. 3. (20 pts) Use the following thermodynamic data (reported at 298 K and 1 bar) to determine: Substance 4/Hº (kJ/mol) S. (I/K-mol) 4,6° (kJ/mol) N2H4(1) 50.53 121.21 149.4 159.4 N2H4(g) 95.4 Wap 238.9 205.14 191. 610 O2(g) 0 0 N2(g) H2O(1) -237.2 69.91 -285.83 SpA (3a) (5 pts) The molar enthalpy of vaporization of hydrazine N, H. (36) (5 pts) Whether liquid hydrazine vaporizes at 25°C and 1 bar? Hint: Calculate the free energy of vaporization...
The standard enthalpy change for the following reaction is -415 kJ at 298 K. Zn(s) + Ch(g) → ZnCl2() AH° = -415 kJ What is the standard enthalpy change for the reaction at 298 K? ZnCl(s) — Zn(s) + Cl2(g) The standard enthalpy change for the following reaction is -50.6 kJ at 298 K. N2H40 - N2(g) + 2 H2(g) AH° = -50.6 kJ What is the standard enthalpy change for this reaction at 298 K? N2(g) + 2 H2(g)...
4) Calculate the ΔGrxn using the following information. 4 HNO3(g)+5N2H40)- 7 N2(8) +12 H200) -133.9 AH。f (kJ/mol) s°C/mol K) 50.6 -285.8 266.9 121.2 191.6 70.0 A. Determine the enthalpy change 1° for the reaction at 298 K B. Determine aSsurr for the re C. Determine aSsvs for the reaction. D.Find the entropy change of the universe. E. Determine △G"for this reaction. Will this reaction be spontaneous? E. Determine the equilibrium constant Kp at 298K.
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