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Consider the reaction Cr₂O7²-(aq) + I¯(aq) → Cr³+ (aq) + I₂(s). (a) Balance this equation assuming the reaction occurs in acidic solution. (Include states-of-matter under the given conditions in your answer.) chemPad Help XX→→ 2- Cr₂0₂²- (aq) + 14H+(aq) + 61¯(aq) → 2Cr³+(aq) + 31₂(s) + 7H₂O(1) Cr_20_7^2-(aq) + 14H^+(aq) + 61^-(aq)-->2Cr^+3(aq) + 31_2(s) + 7H_20(1) Correct. 0 (b) Using standard reduction potentials, calculate the Ecell, AGO, and K for the reaction at 298.15 K. 0.79 Ecell = AG⁰ = K = Tutorial Greek 1.5e80 X V J X (Use 298.15 as the temperature and round answer to two significant figures) (c) Calculate the cell potential if = 3.64×10−³ M, [Cr₂O7²- ] = 2.40×10−² M, [H+] = 2.29×10-³ M, and [Cr³+] = 4.36×10-² M. V Did you use H+ and H₂O to balance a redox equation in acidic solution? Did you recall the equations relating Eº, AG°, and K?
A voltaic cell utilizes the following oxidation-reduction (redox) reaction. Mg(s) + 2 Ag+ (aq) → Mg2+ (aq) + 2 Ag(s) (a) If the standard cell potential of this cell is +3.172 V, calculate the cell potential at 298.15 K when [Ag+] = 0.263 M and [Mg2+] = 0.00179 M. X V 3 (b) How will the cell potential of the cell change as the reaction proceeds? O It will increase. It will decrease. 123 Tutorial
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