Homework Answers
E0(cell) = E0 (Ag+ / Ag) - E0(Mg^2+ / Mg)
or
E0(cell) = 0.80 + 2.37 = 3.17 V
Mg.................> Mg^2+ + 2e
thus
n = 2
and
we know,
delta G = - nF * E0(cell) = - 2 * 96485 * 3.17 = - 611715 J / mole = - 611.7 KJ / mole (answer)
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can you find this answer at 350K? I know how to find it at
standard conditions!...
Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K....
Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K. AG MPEO 7. Ag (aq) + Mg(s) S Ag(s)+ Mg2 (aq) (a)
Please can I get step solution to question. Answer is provided. 2 The standard reaction Gibbs...
Please can I get step solution to question. Answer is provided.
2 The standard reaction Gibbs energy for K:CrO4(aq) + 2Ag(s) + 2FeCl3(aq) → Ag;CrO4(s) + 2FeCl2(aq) + 2KCI(aq) is-62.5 kJ mol" at 298 K. Calculate the standard emfof the corresponding galvanic cell and (a) (b) the standard potential of the Ag:CrO:] Ag, Cro couple.
problem 9 D . the answer is 99.1 I don’t know how to do problem please...
problem 9 D . the answer is 99.1 I don’t know how to do problem
please show step by step
Problems | 261 E of 9. ng it to anide onsider the following reaction, in which two electrons are transferred from cytochrome-c (reduced) 2cyt c[Fe2+] +pyruvate 2H- 2cyt c[Fe3 + lactate for this reaction at p a. What is b. Calc H 7 and 25°C? ically, ulate the equilibrium constant for the reaction at pH 7 and 25°C. c. Calculate...
Calculate the Gibbs energy change from the standard cell potential following redox reactions at
7. Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350K(a) \(\quad A g^{\prime}(a q)+M g(s) \leftrightharpoons A g(s)+M g^{2 *}(a q)\)(b) \(\mathrm{Cu}^{2 \cdot}(\mathrm{aq})+\mathrm{OH}(\mathrm{aq}) \div \mathrm{Cu}^{+1}(\mathrm{aq})+\mathrm{O}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(1)\)(c) \(\quad \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})+\mathrm{Fe}^{+1}(\mathrm{aq}) \leftrightarrows \mathrm{Fe}^{-2}(\mathrm{aq})+\mathrm{Mg}(\mathrm{s})+\mathrm{OH}^{-1}(\mathrm{aq})\)8. Complete the following table and comment on the spontancity each reaction.
i need the K+ value this question was submitted already but the second answer i got...
i need the K+ value this question was submitted already but
the second answer i got was incorrect.
Calculate the standard change in Gibbs free energy, AGn, for the following reaction at 25.0 °C. Standard Gibbs free energy of formation values can be found here. rxn: KCI K (aq)+ CI (ag) Number kJ/ mol Then, determine the concentration of K*(aq) if the change in Gibbs free energy, AGn, for the reaction is -8.45 kJ/mol. Number M
Calculate the standard change...
nad hi 9. For the following cell at 298 K: (10 pts) Cu(S) Mn(S) MnCl2(aq) (0.0150 M), HCl(aq) (0.10 M) | O2(g) 0.35...
nad hi 9. For the following cell at 298 K: (10 pts) Cu(S) Mn(S) MnCl2(aq) (0.0150 M), HCl(aq) (0.10 M) | O2(g) 0.35 bar) PS) .185 V for the Mn2+/Mn couple and E° = 1.229 V for the O/H20, H couple. Assume the aqueous solutions behave ideally. (a) Write the half reactions and the balanced redox equation. (b) Calculate the standard potential of the cell, E' cell. (C) Calculate the potential of the cell, Ecell. (d) Calculate change in the...
please answer all questions for rate. thank you :) For the following equation: MnO4 (aq) +...
please answer all questions for rate. thank you :)
For the following equation: MnO4 (aq) + Ca(s) → MnO2(s) + Ca?*(aq) Standard Reduction Potential values: Mno. MnO2 = 1.68 V Ca? / Ca = -2.76 V (1) Write balanced half-reaction equations for oxidation and reduction (2) Write the balanced equation for the overall redox reaction (3) Use the two balanced half-reactions and standard reduction potential values to construct a spontaneous galvanic cell, and write the cell notation for the galvanic...
Can someone please help me? I keep getting stuck, I don’t know how to get log...
Can
someone please help me? I keep getting stuck, I don’t know how to
get log on the other side of the equation. I can easily follow
another tutorial, but I can’t figure out the ending and what step I
need to do to get it! This was previously answered by someone else
and was wrong. I need to know HOW to work it out please!
Given the measured cell potential, Ecel, is-0.3555 V at 25 C in the following...
(a) For the following conditions, calculate the change in the Gibbs energy associated with transporting 1...
(a) For the following conditions, calculate the change in the Gibbs energy associated with transporting 1 mole of sodium ions from inside to outside the cell. Is work required or produced? Outside: [Na+] = 130 mM [K+] 5 mM Electrical potential = 0 mV [Na+]= [K 110 mM Electrical potential =-70 mV Temperature 25 °C Inside: 10 mM (b) For the same conditions, calculate the change in the Gibbs energy associated with transporting 1 mole of potassium ions from outside...
the answer is 4.73, but i do not know how he got the answer. thank you!...
the answer is 4.73, but i do not know how he got the answer.
thank you!
(4) The Standard cell potential of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2H+ (aq) = Zn²+ (aq) + H₂lg). with PH2 = 1.0 am and [zn 2] = 0 , the cell potential 0.48M. what is pH in cathodic department?
Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K. AG MPEO 7. Ag (aq) + Mg(s) S Ag(s)+ Mg2 (aq) (a)
Please can I get step solution to question. Answer is provided.
2 The standard reaction Gibbs energy for K:CrO4(aq) + 2Ag(s) + 2FeCl3(aq) → Ag;CrO4(s) + 2FeCl2(aq) + 2KCI(aq) is-62.5 kJ mol" at 298 K. Calculate the standard emfof the corresponding galvanic cell and (a) (b) the standard potential of the Ag:CrO:] Ag, Cro couple.
problem 9 D . the answer is 99.1 I don’t know how to do problem
please show step by step
Problems | 261 E of 9. ng it to anide onsider the following reaction, in which two electrons are transferred from cytochrome-c (reduced) 2cyt c[Fe2+] +pyruvate 2H- 2cyt c[Fe3 + lactate for this reaction at p a. What is b. Calc H 7 and 25°C? ically, ulate the equilibrium constant for the reaction at pH 7 and 25°C. c. Calculate...
7. Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350K(a) \(\quad A g^{\prime}(a q)+M g(s) \leftrightharpoons A g(s)+M g^{2 *}(a q)\)(b) \(\mathrm{Cu}^{2 \cdot}(\mathrm{aq})+\mathrm{OH}(\mathrm{aq}) \div \mathrm{Cu}^{+1}(\mathrm{aq})+\mathrm{O}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(1)\)(c) \(\quad \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})+\mathrm{Fe}^{+1}(\mathrm{aq}) \leftrightarrows \mathrm{Fe}^{-2}(\mathrm{aq})+\mathrm{Mg}(\mathrm{s})+\mathrm{OH}^{-1}(\mathrm{aq})\)8. Complete the following table and comment on the spontancity each reaction.
i need the K+ value this question was submitted already but
the second answer i got was incorrect.
Calculate the standard change in Gibbs free energy, AGn, for the following reaction at 25.0 °C. Standard Gibbs free energy of formation values can be found here. rxn: KCI K (aq)+ CI (ag) Number kJ/ mol Then, determine the concentration of K*(aq) if the change in Gibbs free energy, AGn, for the reaction is -8.45 kJ/mol. Number M
Calculate the standard change...
nad hi 9. For the following cell at 298 K: (10 pts) Cu(S) Mn(S) MnCl2(aq) (0.0150 M), HCl(aq) (0.10 M) | O2(g) 0.35 bar) PS) .185 V for the Mn2+/Mn couple and E° = 1.229 V for the O/H20, H couple. Assume the aqueous solutions behave ideally. (a) Write the half reactions and the balanced redox equation. (b) Calculate the standard potential of the cell, E' cell. (C) Calculate the potential of the cell, Ecell. (d) Calculate change in the...
please answer all questions for rate. thank you :)
For the following equation: MnO4 (aq) + Ca(s) → MnO2(s) + Ca?*(aq) Standard Reduction Potential values: Mno. MnO2 = 1.68 V Ca? / Ca = -2.76 V (1) Write balanced half-reaction equations for oxidation and reduction (2) Write the balanced equation for the overall redox reaction (3) Use the two balanced half-reactions and standard reduction potential values to construct a spontaneous galvanic cell, and write the cell notation for the galvanic...
Can
someone please help me? I keep getting stuck, I don’t know how to
get log on the other side of the equation. I can easily follow
another tutorial, but I can’t figure out the ending and what step I
need to do to get it! This was previously answered by someone else
and was wrong. I need to know HOW to work it out please!
Given the measured cell potential, Ecel, is-0.3555 V at 25 C in the following...
(a) For the following conditions, calculate the change in the Gibbs energy associated with transporting 1 mole of sodium ions from inside to outside the cell. Is work required or produced? Outside: [Na+] = 130 mM [K+] 5 mM Electrical potential = 0 mV [Na+]= [K 110 mM Electrical potential =-70 mV Temperature 25 °C Inside: 10 mM (b) For the same conditions, calculate the change in the Gibbs energy associated with transporting 1 mole of potassium ions from outside...
the answer is 4.73, but i do not know how he got the answer.
thank you!
(4) The Standard cell potential of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2H+ (aq) = Zn²+ (aq) + H₂lg). with PH2 = 1.0 am and [zn 2] = 0 , the cell potential 0.48M. what is pH in cathodic department?
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