Homework Answers
Equilibrium constant = [product]/ [reactant]
= [B] 2/[A]. = ( 0.189)2/0.112
= 0.3189
now , del G = -RTlnK
ln K = ln 0.3189 = -1.14
so del G would be positive for any temperature range . Thus reaction is not spontaneous enthalpically
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11. Consider the following reaction with the equilibrium concentrations written below at 25°C. You notice that...
the correct answer to #11 is supposed to be b but i keep getting c. what...
the
correct answer to #11 is supposed to be b but i keep getting c.
what am i doing wrong? also, the correct answer to #14 is b but i
keep getting d. please explain where i am going wrong. thank
you
11. Consider the reaction in the previous question, what the equilibrium constant would be equal to at 25°C? a) 0.645 AGE-RT enk b) 1.03x10-16 c) 9.64x10-1. 91.2-0008314 (298,15) enk d) 7.03x108 -0.036B-Ink 12. When a reaction is found...
S-Alculate the standard entropy, Δ.xn, of the following reaction at 25.0 °C using the data in thi...
S-Alculate the standard entropy, Δ.xn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, 사mn, îs-44.2 kJ-mol-1 Number Kmol1 Then, calculate the standard Gibbs free energy of the reaction, AG rxn Number k.J mol Finally, determine which direction the reaction is spontaneous as written at 25.0 °C and standard pressure. O forward reverse O both O neither
S-Alculate the standard entropy, Δ.xn, of the following reaction at 25.0 °C using...
Cyngor C OWIODIS OCION In each case, he fills a reaction vessel with some mixture of...
Cyngor C OWIODIS OCION In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 78.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first...
• Calculate AH , AS and AG for the reaction below at 115°C. Before you begin...
• Calculate AH , AS and AG for the reaction below at 115°C. Before you begin calculating, predict signs (+ or -) for enthalpy, entropy, and free energy of reaction. • Is the reaction spontaneous at 115°C? Na 0 (8) + H2O() → NaOH () Na,0 (s) HO (D) NaOH (s) AH°, (kJ/mol) 414.2 -285.8 -427.0 Sº (J/K-mol) 75.1 70.0 64.0
For each system listed in the first column of the table below, decide (if possible) whether the c...
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the Fnot enough information button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour System Change AS 1.0 g of sodium bromide (NaBr) The sodium bromide...
• Calculate AHK AS and AG for the reaction below at 115°C. Before you begin calculating,...
• Calculate AHK AS and AG for the reaction below at 115°C. Before you begin calculating, predict signs (+ or -) for enthalpy, entropy, and free energy of reaction. • Is the reaction spontaneous at 115°C? • Na 0 (8) + H2O (1) → NaOH(S) AH" (kJ/mol) -414.2 Na 0 (s) HIZO (1) NaOH (S) Sº (J/K mol) 75.1 70.0 6 4.0 -285.8 -427. 0
STANDARD ENTHALPY AND ENTROPY CHANGES OF A REACTION INTRODUCTION (1) Part 3, Mes Consider the following...
STANDARD ENTHALPY AND ENTROPY CHANGES OF A REACTION INTRODUCTION (1) Part 3, Mes Consider the following equilibrium system sscc Fe(a)SCNag) FeSCNP(o) The equilibrium constant, K of this system is (2) resCN KTeSCN Finding K for this system using a colouurimeter and absorhance values has already been described in the "Determination of an Equilibrium Constant" experiment. A similar method is used in this experiment, but the temperature is varied so give values of the equilibrium constant at different temperatures. From the...
I need help with 11 and 12 please. Data Table Mixture NaCl (s) + H2O (1)...
I need help with 11 and 12 please.
Data Table Mixture NaCl (s) + H2O (1) T (initial) T, (final) AT (T-T) -.20 25.00 24.80 NaNO, (s) + H2O (1) 24.99 24.11 -.88 NaCH,COO + H2O (1) 24.99 25.91 .82 Use your experimental data to answer the following questions: 7. Calculate AT (AT = T2-T) for each mixture and record the results in the data table. 8. An exothermic process releases heat (warms up), and an endothermic process absorbs heat...
Chemie Heterogeneous Reaction Chemical reactions may be envisioned in terms of reactants and products and written...
Chemie Heterogeneous Reaction Chemical reactions may be envisioned in terms of reactants and products and written in the general form A +bB - C +dD Reactants Products The equilibrium constant may be expressed in the form K - LORD up or K, - P2 where [C] represents the molar concentration of Catequilibrium. For a given reaction, the concentrations at equilibrium would have to be determined experimentally. In application, there are practical cases where some of the reactants and/or products do...
and HCO 2. Carbonated beverages are acidic because CO, reacts with water to form CO2 (g)...
and HCO 2. Carbonated beverages are acidic because CO, reacts with water to form CO2 (g) + H2O (1) ---> H(aq) + HCO, (aq) For this reaction, AH = -12 kJ/mole and K. = 1.4x108 at 25°C. For HCO, (aq), S = 95J/mole K, AG = -587 kJ/mole a. You take your soda out of your cold refrigerator and let it warm up to room temperature (250C). Heat is a in this reaction so as the temperature increases, the reaction...
the
correct answer to #11 is supposed to be b but i keep getting c.
what am i doing wrong? also, the correct answer to #14 is b but i
keep getting d. please explain where i am going wrong. thank
you
11. Consider the reaction in the previous question, what the equilibrium constant would be equal to at 25°C? a) 0.645 AGE-RT enk b) 1.03x10-16 c) 9.64x10-1. 91.2-0008314 (298,15) enk d) 7.03x108 -0.036B-Ink 12. When a reaction is found...
S-Alculate the standard entropy, Δ.xn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, 사mn, îs-44.2 kJ-mol-1 Number Kmol1 Then, calculate the standard Gibbs free energy of the reaction, AG rxn Number k.J mol Finally, determine which direction the reaction is spontaneous as written at 25.0 °C and standard pressure. O forward reverse O both O neither
S-Alculate the standard entropy, Δ.xn, of the following reaction at 25.0 °C using...
Cyngor C OWIODIS OCION In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 78.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first...
• Calculate AH , AS and AG for the reaction below at 115°C. Before you begin calculating, predict signs (+ or -) for enthalpy, entropy, and free energy of reaction. • Is the reaction spontaneous at 115°C? Na 0 (8) + H2O() → NaOH () Na,0 (s) HO (D) NaOH (s) AH°, (kJ/mol) 414.2 -285.8 -427.0 Sº (J/K-mol) 75.1 70.0 64.0
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the Fnot enough information button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour System Change AS 1.0 g of sodium bromide (NaBr) The sodium bromide...
• Calculate AHK AS and AG for the reaction below at 115°C. Before you begin calculating, predict signs (+ or -) for enthalpy, entropy, and free energy of reaction. • Is the reaction spontaneous at 115°C? • Na 0 (8) + H2O (1) → NaOH(S) AH" (kJ/mol) -414.2 Na 0 (s) HIZO (1) NaOH (S) Sº (J/K mol) 75.1 70.0 6 4.0 -285.8 -427. 0
STANDARD ENTHALPY AND ENTROPY CHANGES OF A REACTION INTRODUCTION (1) Part 3, Mes Consider the following equilibrium system sscc Fe(a)SCNag) FeSCNP(o) The equilibrium constant, K of this system is (2) resCN KTeSCN Finding K for this system using a colouurimeter and absorhance values has already been described in the "Determination of an Equilibrium Constant" experiment. A similar method is used in this experiment, but the temperature is varied so give values of the equilibrium constant at different temperatures. From the...
I need help with 11 and 12 please.
Data Table Mixture NaCl (s) + H2O (1) T (initial) T, (final) AT (T-T) -.20 25.00 24.80 NaNO, (s) + H2O (1) 24.99 24.11 -.88 NaCH,COO + H2O (1) 24.99 25.91 .82 Use your experimental data to answer the following questions: 7. Calculate AT (AT = T2-T) for each mixture and record the results in the data table. 8. An exothermic process releases heat (warms up), and an endothermic process absorbs heat...
Chemie Heterogeneous Reaction Chemical reactions may be envisioned in terms of reactants and products and written in the general form A +bB - C +dD Reactants Products The equilibrium constant may be expressed in the form K - LORD up or K, - P2 where [C] represents the molar concentration of Catequilibrium. For a given reaction, the concentrations at equilibrium would have to be determined experimentally. In application, there are practical cases where some of the reactants and/or products do...
and HCO 2. Carbonated beverages are acidic because CO, reacts with water to form CO2 (g) + H2O (1) ---> H(aq) + HCO, (aq) For this reaction, AH = -12 kJ/mole and K. = 1.4x108 at 25°C. For HCO, (aq), S = 95J/mole K, AG = -587 kJ/mole a. You take your soda out of your cold refrigerator and let it warm up to room temperature (250C). Heat is a in this reaction so as the temperature increases, the reaction...
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