Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron- transfer reaction. Zn2+ (aq) + Mg(s). species oxidized oxidizing agent Zn(s) + Mg2+ (aq) species reduced Submit Answer reducing agent As the reaction proceeds, electrons are transferred from Retry Entire Group 9 more group attempts remaining to

Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron- transfer reaction. Zn2+ (aq) + Mg(s). species oxidized oxidizing agent Zn(s) + Mg2+ (aq) species reduced Submit Answer reducing agent As the reaction proceeds, electrons are transferred from Retry Entire Group 9 more group attempts remaining to

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter22: An Introduction To Electroanalytical Chemistry

Section: Chapter Questions

Problem 22.18QAP

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1. What is the gravimetric factor of SO3 in BaSO4? 2. What is the normality of an oxidizing agent of a solution of potassium dichromate (K2Cr2O7) containing 8.906 g per 200 mL in the presence of acid? (Cr2O7-2 + 6Fe+3 + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O) NOTE: Present complete solution with corresponding units.
Two Copper strips were used to determine the effect of supporting electrolyte used on the change in mass. Three different experiments were conducted for 5mins where 0.5A current is applied throughout the experiment. In the first experiment two copper strips were immersed in 3.080g of Cu (NO3)2 dissolved in 25mL of DI water and tested for 5mins while applying current 0.5A. The weight of one copper strip act as an anode is taken before the reaction and after the reaction to calculate the change in mass due to different applied current. Same process is repeated with 25ml 0.5 M CuSO4 and25ml 0.5 M CuCl2 for 5 mins Using Faraday’s equation (Eq 1), calculate the theoretical mass and Compares the theoretical mass (mg) of copper and the actual mass deposited (obtained from the electrolysis, ∆m) by calculating the %error at different times. Discuss the observed results. Q = I x t = nFN Electrolyte Initial mass of anode (mg) Final mass of anode (mg) Cu (NO3)2 2941 2893…
Ochem help with prelab The experiment is attached and involves the reduction of a nitro group to an amine The Chemicals are: 200 mg of m-nitroacetophenone 400 mg of granular tin 4 mL of 6M hydrochloric acid 30% sodium hydroxide Need help with the prelab which requires... A. Write the balanced equations for both half-reactions of the redox and then the overall balanced redox equation B. Determine the limiting reagent and the theoretical yield of amine
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Which of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods. A). I, II and V B). I, II, IV and V C). I, III and IV D.) II, IV and V
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Cyclic voltammetry (CV) is a powerful and popular electrochemical technique commonly employed to investigate the reduction and oxidation processes of molecular species
Which is equivalent to 2,500 ppm Cu2+?Molecular Weight: Cu (63.55) a. 0.07868 N (in precipitation reaction) b. 0.07868 N (in redox into Cu+)
Two Copper strips were used to determine the effect of electrolysis time and immersed in 3.080g of Cu (NO3)2dissolved in 25mL of DI water. The weight of one copper strip act as an anode is taken before the reaction and after the reaction to calculate the change in mass due to different applied current. The current is applied for 5mins for every reptation. Current (A) 0.5 1.0 1.5 2.0 Initial mass of strip (mg) 2941 3390 2.893 2.738 Final mass of strip (mg) 2893 3297 2.738 2.573 Mass change Dm (mg) 48 93 155 165 The theoretical mass of copper deposited on supplying different current: Michael Faraday equation: Q = I x t = nFN Calculate the theoretical mass that should be obtained at each applied current and Compares the theoretical mass (mg) of copper and the actual mass deposited (obtained from the electrolysis, ∆m) by calculating the %error at different times. Briefly discuss the observed results. Is there any trend observed?