1. Which of the following reactions would be spontaneous at standard state conditions and 25C? EXPLAIN your answer.
a. Cu2+ + 2Br- ---> Br2(aq) + Cu
b. Br2(aq) + 2Cl- ---> Cl2(aq) + 2Br-
c. Fe + Cu2+ ---> Fe2+ + Cu
2. What would happen to the cell potential for the reaction below if the concentration of Cr3+ were reduced to .010M? Explain your answer and show your work.
2Cr + 3Cu2+ ---> 2Cr3+ + 3Cu
a. It would go up by .02 volts.
b. It would go down by .02 volts.
c. It would go up by .04 volts.
d. It would go down by .04 volts.
e. It would not change.
1. Which of the following reactions would be spontaneous at standard state conditions and 25C? EXPLAIN...
Which one of the following reactions is spontaneous (in the direction given) under standard elecrochemical conditions? A. Pb2+ + 2I- --> Pb + I2 B. Cu2+ + Fe ---> Cu + Fe2+ C. 2Au + Pt2+ --> 2Au+ + Pt D. Mg2+ + 2Br- --> Mg + Br2 E. 2Hg + 2Cl- +2H+ --> Hg2Cl2 + H2
Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to be oxidised by O2 (g) in acidic aqueous solution? Select one: a. Br2 (l) b. Br- (aq) c. Ni2+ (aq) d. Ag (s) e. Cu2+ (aq) Cathode (Reduction) Half-Reaction Standard Potential E° (volts) Li+(aq) + e- -> Li(s) -3.04 K+(aq) + e- -> K(s) -2.92 Ca2+(aq) + 2e- -> Ca(s) -2.76 Na+(aq) + e- -> Na(s) -2.71 Mg2+(aq) + 2e- -> Mg(s) -2.38 Al3+(aq)...
Write net equation for the spontaneous redox reaction and determine the standard cell potential that results when each of the following redox couples are connected in an electrochemical cell. Instructions: Enter all substances in the order listed at the top of the column. Use a carot to indicate a superscript, but do nothing for subscripts. Use a hyphen + greater than (->) for yields. Click on the eye symbol to check your formatting. 1. + 20/24 points Previous Answers My...
Your Answer has to be 100% correct. Check your calculation A) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 5.48×10-4 atm, the Cl- concentration is 1.47M, and the Fe2+ concentration is 1.07M ? Cl2(g) + Fe(s)---> 2Cl-(aq) + Fe2+(aq) Answer: _____ V The cell reaction as written above is spontaneous for the concentrations given: _____ ( TRUE/FALSE ) B) What is the calculated value...
help with these please Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2 concentration is 9.24x104 M and the Cr3 concentration is 1.47 M ? 3Cu2 (aq)+2Cr(s)3Cu(s) + 2Cr (aq) V Answer: The cell reaction as written above is spontaneous for the concentrations given: What is the binding energy in kJ/mol nucleons for silver-107? kJ/mol...
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...
A) B) C) C) Enter electrons as e. A voltaic cell is constructed in which the anode is a CuCu2+ half cell and the cathode is a II, half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: In the...
please help the standrad reduction provided down What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 9.24x10 + M and the Cr3+ concentration is 1.47 M? 3Cu2+ (aq) + 2Cr(s) Answer: 3Cu(s) + 2Cr +(aq) v The cell reaction as written above is spontaneous for the concentrations given: What is the calculated value of the cell potential at 298K for an electrochemical cell with the...
Given the following half reactions what is the voltage of the galvanic cell that would result from their combination [maximum positive voltage and spontaneous reaction). Show work. E° (volts) -0.74 Cr3+ (aq) + 3e Cu2+ (aq) + 2e → → Cr (8) Cu (s) +0.34 And what is the overall reaction that results after the half reactions are combined to cancel all electrons. Show work. And fill in the following abbreviated cell to represent the actual galvanic cell from above.
12. Using two half reactions that have NEGATIVE standard reduction potentials results results in a battery that... Reduction Half-Reaction F2(g) + 2e →2F(aq) S2082 (aq) + 2e- → 25042 (aq) O2(g) + 4H+ (aq) + 4e → 2H2O(1) Br2(1) + 2e + 2Br (aq) Agt(aq) + e → Ag(s) Fe3+ (aq) + e- → Fe2+ (aq) 126) + 2e → 21 (aq) Cu2+ (aq) + 2e → Cu(s) Sn4+ (aq) + 2e → Sn2+ (aq) S(s) + 2H+ (aq) +...