The species getting oxidized by 1M HBr needs to be identified. Concept introduction: A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction . The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized. An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s. Spontaneity of a reaction is dependent on the free energy sign that is Δ G o . It should be negative for a reaction to be spontaneous. Since, Δ G = − n F E o Here, n = number of electrons involved in reaction and F is faraday constant. If the value of E° for a reaction is positive, then the reaction occurs spontaneous.
The species getting oxidized by 1M HBr needs to be identified. Concept introduction: A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction . The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized. An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s. Spontaneity of a reaction is dependent on the free energy sign that is Δ G o . It should be negative for a reaction to be spontaneous. Since, Δ G = − n F E o Here, n = number of electrons involved in reaction and F is faraday constant. If the value of E° for a reaction is positive, then the reaction occurs spontaneous.
Solution Summary: The author explains that the species getting oxidized by 1M HBr needs to be identified.
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
Chapter 17, Problem 46QAP
Interpretation Introduction
Interpretation:
The species getting oxidized by 1M HBr needs to be identified.
Concept introduction:
A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction. The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized.
An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s.
Spontaneity of a reaction is dependent on the free energy sign that is ΔGo. It should be negative for a reaction to be spontaneous.
Since,
ΔG=−nFEo
Here, n = number of electrons involved in reaction and F is faraday constant.
If the value of E° for a reaction is positive, then the reaction occurs spontaneous.
19. The salt, Ca(CN)2, would give an aqueous solution that is
(a) acidic
(b) basic
(c) neutral
(d) none of these
The arsenic in a 1.22-g sample of a pesticide was converted to As by suitable chemical treatment. It was then titrated using Ag+ to form Ag3AsO4 as a precipitate. (a) What is the oxidation state of As in As ? (b) Name Ag3AsO4 by analogy to the corresponding compound containing phosphorus in place of arsenic. (c) If it took 25.0 mL of 0.102 M Ag+ to reach the equivalence point in this titration, what is the mass percentage of arsenic in the pesticide?
Consider the following balanced redox reaction: 16H+(aq) + 2MnO4-(aq) + 10Cl-(aq) → 2Mn2+(aq) + 5Cl2(g) + 8H2O(l)(a) Which species is being oxidized?(b) Which species is being reduced?(c) Which species is the oxidizing agent?(d) Which species is the reducing agent?(e) From which species to which does electron transfer occur?(f ) Write the balanced molecular equation, with K+ and SO42- as the spectator ions.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell