Nonspontaneous under standard conditions
Consider the reaction:
Ag+ (aq) + Cl- (aq) → AgCl (s)
Given the following table of thermodynamic data,
determine the temperature (in °C) above which the reaction is nonspontaneous under standard conditions.
A) 1640
B) 150
C) 1230
D) 432
E) 133
Homework Answers
ΔH = -127-(105.9-167.2) = -65.7kJ
ΔS = 96.11 - ( 56.5+73.93) = -34.32J
ΔG = ΔH - TΔS
0 = -65.7 - T(-34.32)/1000
T = 1641.80C
so option (a) is correct.
please helpppp!!! 7) The standard cell potential (E cell) f for the reaction below i ls...
please helpppp!!!
7) The standard cell potential (E cell) f for the reaction below i ls -0 43 V. The cell potential for this at best cong (6 polnts) Ag Acid 6 natch the H idding 6e e cancel e, pposite pposite (e) e ancel is the he por Poten 8) The standard cell potential (E-cell) of the reaction below is .0.126 V. The value of ΔG" for the reaction is Pb (o) 2H (aq)Pb2+ (aq) H2 (g) vith (6...
19.03 pts Question 10 Use the standard reduction potenital to calculate equilibrium constants for the following...
19.03 pts Question 10 Use the standard reduction potenital to calculate equilibrium constants for the following reaction at 298.15 K. AgCl (s) Ag+ (aq) +Cl- (aq) Ag+ (aq) +Ag(s) E° = 0.7996 V AgCl(s) + e - Ag(s) + CH- (aq) E° = 0.22233 V O K=5.2 x 105 spontaneous O K = 3.8 x 10"nonspontaneous K - 1.7 x 10-10 nonspontaneous
Since the computed value for AG is positive, the reaction is nonspontaneous under these conditions. Check...
Since the computed value for AG is positive, the reaction is nonspontaneous under these conditions. Check Your Learning Calculate the free energy change for this same reaction at 875 °C in a 5.00 L mixture containing 0.100 mol of each gas. Is the reaction spontaneous under these conditions? ANSWER: AG +45.1 kJ/mol; no Calculating AG under Nonstandard Conditions What is the free energy change for the process shown here under the specified conditions? T 25 °C, PN, 0.870 atm, PH=0.250...
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0...
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH,CI() = NH(aq) + Cl(aq) AGxn = -7.7 kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGrxn , for the reaction is –9.53 kJ/mol. [NH] = 0.72 Consider a general reaction enzyme A(aq) = B(aq) The AG® of the reaction is -4.880 kJ mol-....
Since the computed value for AG is positive, the reaction is nonspontaneous under these conditions. Check...
Since the computed value for AG is positive, the reaction is nonspontaneous under these conditions. Check Your Learning Calculate the free energy change for this same reaction at 875 °C in a 5.00 L mixture containing 0.100 mol of each gas. Is the reaction spontaneous under these conditions? ANSWER: AG = +45.1 kJ/mol; no EXAMPLE 16.12 Calculating AG under Nonstandard Conditions What is the free energy change for the process shown here under the specified conditions? T = 25 °C,...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State wheth...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
QUESTION 45 For the reaction Ag+ (aq) + Cr (aq) - AOCI (5) Given the following...
QUESTION 45 For the reaction Ag+ (aq) + Cr (aq) - AOCI (5) Given the following table of thermodynamic data, Substance AHF (k]/mol) S (I/mol.K) Ag+ (aq) 105.90 73.93 a- (aq) -167.2 56.5 AgCl (5) -127.0 96.11 determine the temperature at which the reaction becomes spontaneous O 1640 K O 1914 K 0 432K O 850K O 522K QUESTION 46 What is the low for a solution at 25°c that has a pH of 8 647 O 1.2 x 10-10...
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Consider the following reaction: CACO3(s) CaO (s) + CO2 (g). Estimate AG for this reaction at each of the following temperatures. (Assume that AH° and AS do not change too much within the given temperature range.) Part A 290 K Part B 1095 K Part C 1475 K
Consider the electrochemical cell operating under standard conditions Co | Co2+ || Ag+ | Ag Which...
Consider the electrochemical cell operating under standard conditions Co | Co2+ || Ag+ | Ag Which of the following statements is/are correct? 1. The cell EMF is 0.52 volts 2. The spontaneous cell reaction is 2 Ag(s)+ Co2+(aq)→2 Ag+(aq)+ Co(s) 3. The Ag | Ag+ electrode is the anode 4. The spontaneous electron flow in the external circuit is from the Co terminal to the Ag terminal A.2,3 & 4 only B. none C. 3 & 4 only D. 1...
Using the following standard reduction potentials: Fe3+ (aq) + e. → Fe2+ (aq) Eo = +0.77...
Using the following standard reduction potentials: Fe3+ (aq) + e. → Fe2+ (aq) Eo = +0.77 V Pb2+ (aq) + 2 e. → Pb(s) E。--0.13 V Calculate the standard cell potential for the galvanie cell reaction given below, and determine whether or not this reaction is spostaneous under standard conditions. Pb2+ (aq) + 2 Fe2+ (aq) → 2 Fe3+ (aq) + Pb(s) ⓔ A. E.-0.90 V, nonspontaneous OB. E-0.90 V, spontaneous C. Eo +0.90 V, nonspontaneous OD0.90 V, spontaneous
please helpppp!!!
7) The standard cell potential (E cell) f for the reaction below i ls -0 43 V. The cell potential for this at best cong (6 polnts) Ag Acid 6 natch the H idding 6e e cancel e, pposite pposite (e) e ancel is the he por Poten 8) The standard cell potential (E-cell) of the reaction below is .0.126 V. The value of ΔG" for the reaction is Pb (o) 2H (aq)Pb2+ (aq) H2 (g) vith (6...
19.03 pts Question 10 Use the standard reduction potenital to calculate equilibrium constants for the following reaction at 298.15 K. AgCl (s) Ag+ (aq) +Cl- (aq) Ag+ (aq) +Ag(s) E° = 0.7996 V AgCl(s) + e - Ag(s) + CH- (aq) E° = 0.22233 V O K=5.2 x 105 spontaneous O K = 3.8 x 10"nonspontaneous K - 1.7 x 10-10 nonspontaneous
Since the computed value for AG is positive, the reaction is nonspontaneous under these conditions. Check Your Learning Calculate the free energy change for this same reaction at 875 °C in a 5.00 L mixture containing 0.100 mol of each gas. Is the reaction spontaneous under these conditions? ANSWER: AG +45.1 kJ/mol; no Calculating AG under Nonstandard Conditions What is the free energy change for the process shown here under the specified conditions? T 25 °C, PN, 0.870 atm, PH=0.250...
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH,CI() = NH(aq) + Cl(aq) AGxn = -7.7 kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGrxn , for the reaction is –9.53 kJ/mol. [NH] = 0.72 Consider a general reaction enzyme A(aq) = B(aq) The AG® of the reaction is -4.880 kJ mol-....
Since the computed value for AG is positive, the reaction is nonspontaneous under these conditions. Check Your Learning Calculate the free energy change for this same reaction at 875 °C in a 5.00 L mixture containing 0.100 mol of each gas. Is the reaction spontaneous under these conditions? ANSWER: AG = +45.1 kJ/mol; no EXAMPLE 16.12 Calculating AG under Nonstandard Conditions What is the free energy change for the process shown here under the specified conditions? T = 25 °C,...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
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Consider the following reaction: CACO3(s) CaO (s) + CO2 (g). Estimate AG for this reaction at each of the following temperatures. (Assume that AH° and AS do not change too much within the given temperature range.) Part A 290 K Part B 1095 K Part C 1475 K
Using the following standard reduction potentials: Fe3+ (aq) + e. → Fe2+ (aq) Eo = +0.77 V Pb2+ (aq) + 2 e. → Pb(s) E。--0.13 V Calculate the standard cell potential for the galvanie cell reaction given below, and determine whether or not this reaction is spostaneous under standard conditions. Pb2+ (aq) + 2 Fe2+ (aq) → 2 Fe3+ (aq) + Pb(s) ⓔ A. E.-0.90 V, nonspontaneous OB. E-0.90 V, spontaneous C. Eo +0.90 V, nonspontaneous OD0.90 V, spontaneous
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