(a)
Interpretation:
The oxidation state of all atoms in
Concept Introduction:
The
Oxidation is the process in which either loss of electrons, oxidation number increases, or loss of hydrogen atoms takes place. An element is oxidized, when oxidation number increases.
Reduction is the process in which either gain of electrons, oxidation number decreases, or gain of hydrogen atoms takes place. An element is reduced, when oxidation number decreases.
Oxidation state is also known as oxidation number. It is defined as the numbers which are assign to the elements in a chemical combination and number represents the electrons which an atom can share, lose or gain to form
Therefore, transfer of electrons refers to the oxidation state.
(b)
Interpretation:
The oxidation state of all atoms in
Concept Introduction:
The chemical reaction in which both oxidation and reduction process takes place is known as redox reaction. In this reaction, transfer of electrons takes place among the elements.
Oxidation is the process in which either loss of electrons, oxidation number increases, or loss of hydrogen atoms takes place. An element is oxidized, when oxidation number increases.
Reduction is the process in which either gain of electrons, oxidation number decreases, or gain of hydrogen atoms takes place. An element is reduced, when oxidation number decreases.
Oxidation state is also known as oxidation number. It is defined as the numbers which are assign to the elements in a chemical combination and number represents the electrons which an atom can share, lose or gain to form chemical bonding with an atom of another element.
Therefore, transfer of electrons refers to the oxidation state.
(c)
Interpretation:
The oxidation state of all atoms in
Concept Introduction:
The chemical reaction in which both oxidation and reduction process takes place is known as redox reaction. In this reaction, transfer of electrons takes place among the elements.
Oxidation is the process in which either loss of electrons, oxidation number increases, or loss of hydrogen atoms takes place. An element is oxidized, when oxidation number increases.
Reduction is the process in which either gain of electrons, oxidation number decreases, or gain of hydrogen atoms takes place. An element is reduced, when oxidation number decreases.
Oxidation state is also known as oxidation number. It is defined as the numbers which are assign to the elements in a chemical combination and number represents the electrons which an atom can share, lose or gain to form chemical bonding with an atom of another element.
Therefore, transfer of electrons refers to the oxidation state.
(d)
Interpretation:
The oxidation state of all atoms in
Concept Introduction:
The chemical reaction in which both oxidation and reduction process takes place is known as redox reaction. In this reaction, transfer of electrons takes place among the elements.
Oxidation is the process in which either loss of electrons, oxidation number increases, or loss of hydrogen atoms takes place. An element is oxidized, when oxidation number increases.
Reduction is the process in which either gain of electrons, oxidation number decreases, or gain of hydrogen atoms takes place. An element is reduced, when oxidation number decreases.
Oxidation state is also known as oxidation number. It is defined as the numbers which are assign to the elements in a chemical combination and number represents the electrons which an atom can share, lose or gain to form chemical bonding with an atom of another element.
Therefore, transfer of electrons refers to the oxidation state.
(d)
Interpretation:
The oxidation state of all atoms in
Concept Introduction:
The chemical reaction in which both oxidation and reduction process takes place is known as redox reaction. In this reaction, transfer of electrons takes place among the elements.
Oxidation is the process in which either loss of electrons, oxidation number increases, or loss of hydrogen atoms takes place. An element is oxidized, when oxidation number increases.
Reduction is the process in which either gain of electrons, oxidation number decreases, or gain of hydrogen atoms takes place. An element is reduced, when oxidation number decreases.
Oxidation state is also known as oxidation number. It is defined as the numbers which are assign to the elements in a chemical combination and number represents the electrons which an atom can share, lose or gain to form chemical bonding with an atom of another element.
Therefore, transfer of electrons refers to the oxidation state.
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Introductory Chemistry: A Foundation
- Galvanic Cell Using Differents Salts The electrodes used in the galvanic cell are graphite and aluminium. Anode : Aluminium Cathode : Graphite Results : Salt used Trial 1 Trial 2 NaCl 1.05 1.12 KI 1.17 1.07 NaHCO3 0.84 1.04 Question : What is the half-cell equation of cathode and anode. How do you determine the cathode and anode in the equation?arrow_forwardRedox equation of photosynthesis balanced show workingarrow_forwardWhich metals can displace nickel from an aqueous solution but not manganese? All possible answer plz.arrow_forward
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- Reaction: CrO42-(aq)+2H+(aq) <--> Cr2O72-(aq)+H2O(l) YELLOW ORANGE a) Under what conditions will Cr2O72-(aq) predominate? explain / defend your answer choice. b) is this a redox reaction? explain/ defend your answer.arrow_forwardFor the redox reaction given below complete the following: Cr2O7-2+ H+ +FeCl2→ Cr+3 + FeCl3 + H2O (a) What is the oxidation no. of Cr in Cr2O7-2? Answer 1 (b) What is the oxidation no. of Fe in FeCl2 ? Answer 2 (c) Find the element oxidized Answer 3 (d) Find the element Reduced Answer 4 (e) Find the Oxidizing Agent Answer 5 (f) Find the Reducing Agentarrow_forwardWhat is the equilibrium constant for the following redox reaction in acidic solution? Mn^2+(aq) + H2C2O4(aq) = 2CO2(aq) + Mn(s) + 2H+(aq) a. 5.0*10^21 b. 5.0*10^16 c. 5.0*10^8 d. 5.0*10^-12 e. 5.0*10^-24 (Answer is e. but why?)arrow_forward
- Determine the overall balanced equation for the redox reaction below. Assume that it takes place within a basic solution and that all species are aqueous. What are the coefficients for hydroxide ion & X2 once balanced? Hint – X gets both oxidized & reduced. X2 → X– + XO3– Group of answer choices X2 = 1, OH– = 2 X2 = 2, OH– = 5 X2 = 1, OH– = 6 X2 = 3, OH– = 6 X2 = 3, OH– = 3arrow_forwardANSWER ASAP PLEASE THANK YOU Consider R2+ at standard conditions. What is the Eocell (in volts)? Final answer: two decimal places; include negative sign whenever applicable; no unit necessary. Use data given in Table 1. 2R3+(aq) + 2J-(aq) → 2R2+(aq) + J2(s) hypothetical reaction Table 1. Standard Reduction Potentials at 25oC of Some Hypothetical Substances A3+ + 3e- → A Eo = + 1.4 V X2+ + 2e- → X Eo = - 2.87 V R3+ + e- → R2+ Eo = + 0.95 V J2 + 2e- → 2J- Eo = + 0.23 V L2+ + 2e- → L Eo = - 2.36 V T2+ + 2e- → T Eo = - 0.14 Varrow_forwardOxidation/Reduction Practice:arrow_forward
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