None For each of the reactions shown, determine the element being oxidized and the element being reduced: Input the element symbolShow work of all reactionswith explanation needed.don't give Handwrittenansweronly without a charge.a) Re04 +10103 + ReOxidized =Write your response here...Reduced =Write your response here...b) Pb2++103 →PbO2+12Oxidized =Write your response here...Reduced =Write your response here...c) H2O2 + Cr2020₂+ Cr³+Oxidized =Write your response here...Reduced =Write your response here...

Oxidation number rules : Any element in its uncombined state has an oxidation number of 0. The…

Answered: For each of the reactions shown,…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter19: Redox Reactions

Section: Chapter Questions

Problem 89A

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Similar questions

Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required. (a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an appropriate acid) (b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction (c) gaseous H2S from solid Zn and S via a two-step process (first a redox reaction between the starting materials, then reaction of the product with a strong acid)
The Hall process is an important method by which pure aluminum is prepared from its oxide (alumina, Al2O3 ) by indirect reaction with graphite (carbon). Balance the following equation, which is a simplified representation of this process. m:math>Al2O3(s)+C(s)Al(s)+CO2(g)
A common demonstration in chemistry courses involves adding a tiny speck of manganese(IV) oxide to a concentrated hydrogen peroxide, H2O2 , solution. Hydrogen peroxide is unstable, and it decomposes quite spectacularly under these conditions to produce oxygen gas and steam (water vapor). Manganese(IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction. Write the balanced equation for the decomposition reaction of hydrogen peroxide.
4.3 Explain the difference between complete and incomplete combustion.
If electricity of sufficient voltage is passed into a solution of potassium iodide in water, a reaction takes place in which elemental hydrogen gas and elemental iodine are produced, leaving a solution of potassium hydroxide. Write the unbalanced equation for this process.
You have probably had the unpleasant experience of discovering that a flashlight battery has gotten old and begun to leak. Is there evidence that this change is due to a chemical reaction?
The element carbon undergoes many inorganic reactions, as well as being the basis for the field of organic chemistry. Write balanced chemical equations for the reactions of carbon described below. l type='a'> Carbon burns in an excess of oxygen (for example. in the air) to produce carbon dioxide. If the supply of oxygen is limited, carbon will still burn but will produce carbon monoxide rather than carbon dioxide. molten lithium metal is treated with carbon, lithium car bide, Li2C2 , is produced. i>Iron(II) oxide reacts with carbon above temperatures of about 700 °C to produce carbon monoxide gas and molten elemental iron. i>Carbon reacts with fluorine gas at high temperatures to make carbon tetrafluoride.
When heated to 700—800 C, diamonds, which are pure carbon, are oxidized by atmospheric oxygen. (They burn!) Write the balanced equation for this reaction.
For each reaction, indicate which elements are oxidized and which are reduced: a.2Al+3CU2+2Al3++3Cub.2H++NiNi2++H2c.2I-+Cl2I2+2Cl-
Write skeleton equations for the following reactions. ammoniumphosphate(aq)+chromium(III)bromide(aq)ammoniumbromide(aq)+chromium(III)phosphate(s) chromium(VI)hydroxide(s)chromium(VI)oxide(s)+water(l) aluminum(s)+copper(I)chloride(aq)aluminumchloride(aq)+copper(s) potassiumiodide(aq)+mercury(I)nitrate(aq)potassiumnitrate(aq)+mercury(I)iodide(s)
Lithium carbonate and iron(III) chloride will undergo a double replacement reaction, producing lithium chloride and what else?

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