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7. Using the following reaction progress diagram, answer the questions below: wiring Energy A G Rxn....
5. How much faster would a reaction be if a catalyst is used that lowers the...
5. How much faster would a reaction be if a catalyst is used that lowers the activation energy from 20.0 kJ/mol to 10.0 kJ/mol? Do the calculation at two temperatures: first at 25.0°C and then at 0.0°C. (20 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ AGRT Ke=e AGⓇ =-nF8° Units/Constants: Volt: 1 V = 1 J/C Faraday: 1 F = 96,485 C/mole Arrhenius Equation:...
2. Using the decay chain for 238U, calculate the amount of time it takes 5.0 kg...
2. Using the decay chain for 238U, calculate the amount of time it takes 5.0 kg of 238U to decay to 2.5 kg. What mass of 206Pb is produced? (5 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ ΔGIRT Ke=e AGⓇ = -nF8° Units/Constants: Volt: 1 V=1/C Faraday: 1 F -96,485 C/mol e Arrhenius Equation: k = Ae Ea/RT R= 8.314 J/mol K Integrated Rate...
help!! (CH3),CBr + 1 → (CH3),CI + Br the following data were collected: [(CH3)3Br] (M) Time...
help!!
(CH3),CBr + 1 → (CH3),CI + Br the following data were collected: [(CH3)3Br] (M) Time (s) 0.600 0 0.424 10.0 0.300 20.0 0.212 30.0 0.150 40.0 Determine the rate law for this reaction and calculate the rate constant. (20 points) E (V) Thermodynamics: AGº - AH-TAS Nernst Equation: 8 = 8°-(RT/nF)InQ AGⓇ--RTINK At 25°C: 8-6° -0.0591/n)logQ AG RT K-e AG° = -nF8° Units/Constants: Volt: 1 V-1 JC Faraday: 1 F -96,485 C/mole Ea/RT Arrhenius Equation: k = Ae R-8.314...
helpp 3. For the hypothetical reaction A+B → C the following rate data (with and without...
helpp
3. For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s ALM B., Muncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 7.14 x 10 0.100 0.100 1.75 x 10 7.14 x 10 0.0500 0.200 1.76 x 10 3.57 x 10 0.0500 0.100 8.80 x 10 3.57 x 10 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction, and the corresponding rate constants. (16...
Fill in the Blanks 0.34 Half Reaction E. (V) Half Reaction Erd® (V) F + 2e...
Fill in the Blanks 0.34 Half Reaction E. (V) Half Reaction Erd® (V) F + 2e →2F 0+ 2H + 2e →H,02 0.68 Ag* + e → Ag Cu* + e → Cu 0.52 Co? + e Co? O2 + 2H,0 + 4e → 40H 0.40 H,O, + 2H + 2e → 2H,0 Cu2+ + 2e → Cu Cet+e → Ces Cu2+ + e → Cut 0.16 PbO, + 4H+ +50,2 +2e → PbSO, + 2H,0 2H* + 2e →...
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction...
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction of Cut with Zn2+ to produce Cu2+ and Zn? E = 0.28 X v Will Cut be able to reduce Zn2+ to Zn? no (yes or no) What is the standard potential for the reaction of Ce3+ with Ag! to produce Ag? Ex= 0.90 x v Will Cell be able to reduce Ag! to Ag? yes (yer or no) Ered (V) 0.68 0.52 0.40...
1. How do I read the half reaction table? 2. If im asked for the best...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e → Ag Co3 + e + CO2- H2O2 + 2H+ + 2e → 2H,0 Ce4+ + e → Ce+ PbO, + 4H+ + SO42- + 2e → PbSO, + 2H,0 Mno, + 4H+ + 3e → MnO2 + 2H,0 2e + 2H+ + 10, → 103 + H2O Mn0, +8H+ + 5e → Mn2+ + 4H,0 Aul+ + 3e → Au Cl2 + 2e...
the first picture is about some useful information, and the second picture is the question that...
the first picture is about
some useful information, and the second picture is the question
that bothers me. I wonder how we know the half-cell reaction of it.
Please explain!!!
TABLE 18.1 | Standard Reduction Potentials at 25°C (298 K) for Many Common Half-Reactions 8° (V) 0.40 0.34 0.27 0.22 0.20 0.16 0.00 Half-Reaction F2 + 2e →2F Ag2+ + e +Agt Co3- + e + CO2- H2O2 + 2H+ + 2e +2H20 Ce+ + e + Ce+ PbO2 +...
For all of the following experiments, under standard conditions, which species could be spontaneously produced? A...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
5. How much faster would a reaction be if a catalyst is used that lowers the activation energy from 20.0 kJ/mol to 10.0 kJ/mol? Do the calculation at two temperatures: first at 25.0°C and then at 0.0°C. (20 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ AGRT Ke=e AGⓇ =-nF8° Units/Constants: Volt: 1 V = 1 J/C Faraday: 1 F = 96,485 C/mole Arrhenius Equation:...
2. Using the decay chain for 238U, calculate the amount of time it takes 5.0 kg of 238U to decay to 2.5 kg. What mass of 206Pb is produced? (5 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ ΔGIRT Ke=e AGⓇ = -nF8° Units/Constants: Volt: 1 V=1/C Faraday: 1 F -96,485 C/mol e Arrhenius Equation: k = Ae Ea/RT R= 8.314 J/mol K Integrated Rate...
help!!
(CH3),CBr + 1 → (CH3),CI + Br the following data were collected: [(CH3)3Br] (M) Time (s) 0.600 0 0.424 10.0 0.300 20.0 0.212 30.0 0.150 40.0 Determine the rate law for this reaction and calculate the rate constant. (20 points) E (V) Thermodynamics: AGº - AH-TAS Nernst Equation: 8 = 8°-(RT/nF)InQ AGⓇ--RTINK At 25°C: 8-6° -0.0591/n)logQ AG RT K-e AG° = -nF8° Units/Constants: Volt: 1 V-1 JC Faraday: 1 F -96,485 C/mole Ea/RT Arrhenius Equation: k = Ae R-8.314...
helpp
3. For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s ALM B., Muncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 7.14 x 10 0.100 0.100 1.75 x 10 7.14 x 10 0.0500 0.200 1.76 x 10 3.57 x 10 0.0500 0.100 8.80 x 10 3.57 x 10 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction, and the corresponding rate constants. (16...
Fill in the Blanks 0.34 Half Reaction E. (V) Half Reaction Erd® (V) F + 2e →2F 0+ 2H + 2e →H,02 0.68 Ag* + e → Ag Cu* + e → Cu 0.52 Co? + e Co? O2 + 2H,0 + 4e → 40H 0.40 H,O, + 2H + 2e → 2H,0 Cu2+ + 2e → Cu Cet+e → Ces Cu2+ + e → Cut 0.16 PbO, + 4H+ +50,2 +2e → PbSO, + 2H,0 2H* + 2e →...
Consider the following species. Cut Ce3+ Ag+ Zn2+ What is the standard potential for the reaction of Cut with Zn2+ to produce Cu2+ and Zn? E = 0.28 X v Will Cut be able to reduce Zn2+ to Zn? no (yes or no) What is the standard potential for the reaction of Ce3+ with Ag! to produce Ag? Ex= 0.90 x v Will Cell be able to reduce Ag! to Ag? yes (yer or no) Ered (V) 0.68 0.52 0.40...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
2.87 Ered® (V) 0.68 0.52 0.40 0.34 0.16 Half Reaction F,+ 2e →2F Ag* + e → Ag Co3 + e + CO2- H2O2 + 2H+ + 2e → 2H,0 Ce4+ + e → Ce+ PbO, + 4H+ + SO42- + 2e → PbSO, + 2H,0 Mno, + 4H+ + 3e → MnO2 + 2H,0 2e + 2H+ + 10, → 103 + H2O Mn0, +8H+ + 5e → Mn2+ + 4H,0 Aul+ + 3e → Au Cl2 + 2e...
the first picture is about
some useful information, and the second picture is the question
that bothers me. I wonder how we know the half-cell reaction of it.
Please explain!!!
TABLE 18.1 | Standard Reduction Potentials at 25°C (298 K) for Many Common Half-Reactions 8° (V) 0.40 0.34 0.27 0.22 0.20 0.16 0.00 Half-Reaction F2 + 2e →2F Ag2+ + e +Agt Co3- + e + CO2- H2O2 + 2H+ + 2e +2H20 Ce+ + e + Ce+ PbO2 +...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
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