6.f. Consider the following coupled redox reaction.O₂ + 2NADH + 2H* = 2H₂O + 2NAD+Calculate AG" (at 310 K) if the standard reduction potentials for O2 andNAD+ are 0.815V and -0.315V respectively.g. If you wanted to shift the above reaction in f. to the left, how would youadjust the pH? Explain briefly.Lab-related questions.a. In lab, you made a 5 M NaCl stock solution. How would you make a 10-mL 0.5 M NaCl solution from your stock solution?i.9 mL 5 M NaCl and 1 mL waterii.5 mL 5 M NaCl and 5 mL wateriii.1 mL 5 M NaCl and 9 mL wateriv.0.1 mL 5 M NaCl and 9.9 mL waterb. In the first week of lab, you made a pH 7.4 phosphate buffer by mixingsome H₂PO4 with HPO4². The pK₂ of H₂PO4 is 7.2. Which of the followingis true?i.ii.iii.iv.7More H₂PO4* needs to be added because the pH > pKaMore HPO4²- needs to be added because the pH > pKaMore H₂PO4 needs to be added because more acid is needed tomaintain a pH of 7.4.More HPO4²- needs to be added because it is more stable.

Answered: Image /qna-images/answer/dd2f2f90-6ac6-45f6-9662-6c184e3e9b04.jpg

f. Consider the following coupled redox reaction. O2 + 2NADH + 2H* = 2H₂O + 2NAD+ Calculate AG" (at 310 K) if the standard reduction potentials for O2 and NAD+ are 0.815V and -0.315V respectively. g. If you wanted to shift the above reaction in f. to the left, how would you adjust the pH? Explain briefly.

f. Consider the following coupled redox reaction. O2 + 2NADH + 2H* = 2H₂O + 2NAD+ Calculate AG" (at 310 K) if the standard reduction potentials for O2 and NAD+ are 0.815V and -0.315V respectively. g. If you wanted to shift the above reaction in f. to the left, how would you adjust the pH? Explain briefly.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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156. Subject :- Chemistry
indTap - Cengage Learni.. Courses Transfer Course Equivalen. OWLV2 | Online teaching Homepage [Review Topics] [References] Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg*(aq) + 2I°(aq)→ Hg(1) + I½(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be O than zero. Submit Answer Retry Entire Group 9 more group attempts remaining Previou Email Instruc Cengage Learning | Cengage Technical Support DII DD F9 F10 F11 F4 ES F6 F7 F8 F3 $ % & 4 5 6 7 8 9
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