6. Write the equation as an ionic equation and net ionic equation. Write the oxidation numbers of each element in the product and reactant. Tell what is being oxidized and what is being reduced. 2 NaNO4 (aq) + 3 K₂SO3(aq) + H₂0 (→ 2 NO2+ 3 K₂SO4 (aq) + 2 NaOH(aq) lonic Equation: Net Ionic Equation: Oxidation states of reactants: K_N_ 0[1]0[2] 0 [3]_Na_S_H___ Oxidation state of products: K_N_0[1] 0 [2] 0 [3] Na S_H_ The element being oxidized is. The element being reduced is
6. Write the equation as an ionic equation and net ionic equation. Write the oxidation numbers of each element in the product and reactant. Tell what is being oxidized and what is being reduced. 2 NaNO4 (aq) + 3 K₂SO3(aq) + H₂0 (→ 2 NO2+ 3 K₂SO4 (aq) + 2 NaOH(aq) lonic Equation: Net Ionic Equation: Oxidation states of reactants: K_N_ 0[1]0[2] 0 [3]_Na_S_H___ Oxidation state of products: K_N_0[1] 0 [2] 0 [3] Na S_H_ The element being oxidized is. The element being reduced is
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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write the equation as an ionic equation and ionic equation. write the oxidation numbers of each element in the product and reactant. Tell what is being oxidized and what is being reduced.
![6. Write the equation as an ionic equation and net ionic equation. Write the oxidation numbers of each
element in the product and reactant. Tell what is being oxidized and what is being reduced.
2 NaNO4 (aq) + 3 K₂SO3(aq) + H₂0 ➜ 2 NO2(g) + 3 K₂SO4 (aq) + 2 NaOH(aq)
lonic Equation:
Net lonic Equation:
Oxidation states of reactants:
K N
0[1]0[2] 0 [3] Na S_H___
Oxidation state of products:
KNO[1] 0 [2] 0 [3] Na S H_
The element being oxidized is
The element being reduced is.
Priority for Oxidation:
F-
H+ [with nonmetals]
0-2
Group 7A-1
Group 6A-2
Group 5A-3](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa4e453a6-0823-4446-b9a7-023500856720%2Fe05e7219-39dc-4e03-8e2a-fb11fef591d9%2Fjmgdlrc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:6. Write the equation as an ionic equation and net ionic equation. Write the oxidation numbers of each
element in the product and reactant. Tell what is being oxidized and what is being reduced.
2 NaNO4 (aq) + 3 K₂SO3(aq) + H₂0 ➜ 2 NO2(g) + 3 K₂SO4 (aq) + 2 NaOH(aq)
lonic Equation:
Net lonic Equation:
Oxidation states of reactants:
K N
0[1]0[2] 0 [3] Na S_H___
Oxidation state of products:
KNO[1] 0 [2] 0 [3] Na S H_
The element being oxidized is
The element being reduced is.
Priority for Oxidation:
F-
H+ [with nonmetals]
0-2
Group 7A-1
Group 6A-2
Group 5A-3
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