Concept:
In redox reactions reduction and oxidation reaction depends on reduction potential. The species having higher reduction potential get reduced and the species having lower reduction potential get oxidized.
Analysis:
The reduction potential of manganese and nickel is as follows:
The reduction potential of nickel is higher than manganese, thus manganese will reduce Ni2+ to Ni, and manganese itself oxidized to magnese ions. On oxidation of magnese to magnese ion, electron will produce and these electrons will be transferred to nickel ion.
In this process, the amount of the nitrate ion in the solution will not change.
Final answer:
The following does not occur :
the amount of the nitrate ion in the solution changes.
Question 14 3 pts A few granules of manganese metal are placed in a solution of...
A few granules of manganese metal are placed in a solution of nickel(II) nitrate. Which of The following does not occur? the manganese is oxidized to manganese ions nickel ion is reduced to nickel metal electrons are transferred from manganese metal to nickel ion O the amount of nitrate ion in the solution changes O all of these occur
Question 8 Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The acid is followed by its K, value. O HOCI, 29 * 10-8 HC6H50, 1.3 * 10-10 o HNO2,4.6 104 HCHO2, 1.8 104 HCIO, 1.1x102 D Question 14 A few granules of manganese metal are placed in a solution of nickel(II) nitrate. Which of The following does not occur? o the manganese is oxidized to manganese ions...
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How many grams of chromium metal will be deposited from a solution that contains Cr^3+ ions if a current of 1.01 A is applied for 40.2 minutes. Answer in______________ grams? How many grams of cobalt metal will be deposited from a solution that contains Co^2+ ions if a current of 0.517 A is applied for 40.5 minutes. Answer in_____________ grams? How many grams of cobalt metal will be deposited from a solution that contains Co^2+ ions if a current of...
Question 3: In a lab experiment, you are tasked with determining the electrochemical reaction that can occur between aqueous hydrochloric acid (HCl)) and solid magnesium metal (Mg). When the magne- sium is placed in solution, gas bubbles begin to appear around the metal and evolve from solution. (a) Write out the two half reactions that occur when the magnesium is placed in the hydrochloric acid solution. Which species is the getting oxidized? Reduced? (b) Which species is acting as the...
Name: Lab Section: 1 2 3 4 5 6 7 8 Report: Redox Reactions 1. Consider the following balanced redox reaction: 2 Li (8) + CuCl(aq) + Cu (8) + 2 LCI (a) a. Write the oxidation number for each element in the spaces below each species. b. Which element is... Oxidized Reduced C. Which reagent is the... Oxidizing agent? Reducing agenti d. Each Li atom (gains / loses) electron(s) and each Custom (gains / loses) e. In the overall...
help with 13, 14, 15, 16
the cal l for the product of the y recovering the product by evaporating to comedy mass on we There betw Fal mass of in metal Mass of the evaporating dish watch glass and in chordeer heng simet Mass of zinc chionde formed You know ma sticker for units Show your calculations for the above w e belle 6. Mass of zinc reacted: om Proces 136.28 ondisi tion 0.8545g 7. Mass of zine chlorides....
The formate ion, (CHO2-), is related to the acetate ion and forms ionic salts with many metal ions. Assume that 11.874 g of M(CHO2)2 (where M represents the atomic symbol for a particular metal) are dissolved in water. When a solution of 0.300 M sodium sulfate is added, a white precipitate forms. The sodium sulfate solution is added until no more precipitate forms, then a few excess milliliters are added. The precipitate is filtered, washed, and dried. It has a...
RODOX EXAMINATION An oxidation-reduction reaction involves the (1) sharing of electrons (3) transfer of electrons (2) sharing of protons (4) transfer of protons In this reaction, CO→ 2 CO + O2 the oxidation number of carbon changes from: (1) 0 to +4 (3) +3 to 0 (2) +2 to +4 (4) +4 to +2 Which balanced equation represents a redox reaction? AgNO3 (aq) +NaCl (aq) →AgCl (s) +NaNO3 (aq) H2CO3 (aq)...
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1. Write net-ionic equations for the following precipitation reactions: a) The reaction between barium nitrate and sulfuric acid. b) The reaction between calcium nitrate and sodium oxalate. 2. Elements A, B, and C exist as the diatomic molecules A2, B2, and C2. All act as oxidizing agents, i.e., they take electrons from other species. In aqueous solution, A2 is green, B2 is yellow, and C2 is red. When they have gained electrons from other species,...