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The correct balanced redox reactions would be as follows:
1.BH4‾(aq) + ClO3‾(aq) → H2BO3‾(aq) + Cl ‾(aq) [basic]
By using the half-reaction method, we will obtain the following:
BH4-(aq) + 8 OH- = H2BO3- + 5H2O + 8 e-
ClO3- + 3H2O + 6 e- = Cl- + 6OH-
The LCM for the 2 half-reactions would be 24. We add these reactions as follows:
3 BH4- + 24 OH- = 3H2BO3- + 15 H2O + 24e-
4 ClO3- + 12 H2O + 24e- = 4Cl- + 24OH-
-----------------------------------------------------------------
3 BH4- + 4ClO3- = 3H2BO3- + 4Cl- + 3H2O
2.CrO42-(aq) + N2O(g) → Cr3+(aq) + NO(g) [acidic]
By the same procedure above,
(CrO4)2- + 8 H+ + 3 e- = Cr3+ + 4 H2O
N2O + H2O = 2 NO + 2 H+ + 2 e-
The LCM would be 6.
2 (CrO4)2- + 16 H+ + 6 e- = 3 Cr3+ + 8 H2O
3 N2O(g) + 3 H2O(l) = 6 NO(g) + 6 H+ + 6 e-
----------------------------------------------------------------------------------
2 (CrO4)2- + 3 N2O + 10 H+ = 3 Cr3+ + 6 NO + 5 H2O
1.BH4‾(aq) + ClO3‾(aq) → H2BO3‾(aq) + Cl ‾(aq) [basic]
By using the half-reaction method, we will obtain the following:
BH4-(aq) + 8 OH- = H2BO3- + 5H2O + 8 e-
ClO3- + 3H2O + 6 e- = Cl- + 6OH-
The LCM for the 2 half-reactions would be 24. We add these reactions as follows:
3 BH4- + 24 OH- = 3H2BO3- + 15 H2O + 24e-
4 ClO3- + 12 H2O + 24e- = 4Cl- + 24OH-
-----------------------------------------------------------------
3 BH4- + 4ClO3- = 3H2BO3- + 4Cl- + 3H2O
2.CrO42-(aq) + N2O(g) → Cr3+(aq) + NO(g) [acidic]
By the same procedure above,
(CrO4)2- + 8 H+ + 3 e- = Cr3+ + 4 H2O
N2O + H2O = 2 NO + 2 H+ + 2 e-
The LCM would be 6.
2 (CrO4)2- + 16 H+ + 6 e- = 3 Cr3+ + 8 H2O
3 N2O(g) + 3 H2O(l) = 6 NO(g) + 6 H+ + 6 e-
----------------------------------------------------------------------------------
2 (CrO4)2- + 3 N2O + 10 H+ = 3 Cr3+ + 6 NO + 5 H2O
The redox reaction has been defined as the reaction that has been oxidizing and reducing the molecules.
The oxidation has been defined as loss of electrons, while reduction has been defined as the gain of electrons.
Balanced chemical equation
A balanced equation has been defined as the one that follows the law of conservation. In the balanced equation, the number of atoms of each reactant has been equal on the product and the reactant side.
The balanced chemical equation has been given as:
[tex]\rm 3\;BH_4^-\;+\;4\;ClO_3^-\;\rightarrow\;3\;H_2BO_3^-\;+\;4\;Cl^-\;+\;3\;H_2O[/tex]
[tex]\rm 2\;(CrO_4)^2^-\;+\;3\;N_2O\;+\;10\;H^+\;\rightarrow\;3\;Cr^3^+\;+\;6\;NO\;+\;5\;H_2O[/tex]
The molecule that has been reducing itself has been the oxidizing agent, while the molecule that oxidizes itself has been the reducing agent.
In the given reaction, [tex]\rm BH_4^-[/tex] and [tex]\rm N_2O[/tex] has been the reducing agent and [tex]\rm ClO_3^-[/tex] and [tex]\rm (CrO_4)^2^-[/tex] has been the oxidizing agent.
Learn more about redox reaction, here:
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