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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.20 - Electrochemistry문제 19b,c
20장, 문제 19b,c

Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (b) NaI(aq) + 3 HOCl(aq) → NaIO3(aq) + 3 HCl(aq) (c) 3 SO(1g) + 2 HNO3(aq) + 2 H2O(l) → 3 H2SO4(aq) + 2 NO(g)

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Determine the oxidation states of each element in the reactants and products.
For NaI, Na is in the +1 oxidation state and I is in the -1 oxidation state.
For HOCl, H is in the +1 oxidation state, O is in the -2 oxidation state, and Cl is in the +1 oxidation state.
For NaIO_3, Na is in the +1 oxidation state, I is in the +5 oxidation state, and O is in the -2 oxidation state.
For HCl, H is in the +1 oxidation state and Cl is in the -1 oxidation state.

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Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between substances, resulting in changes in oxidation states. In these reactions, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. Identifying whether a reaction is a redox process requires analyzing the oxidation states of the elements involved before and after the reaction.
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가이드 코스
01:53
Oxidation and Reduction Reactions

Oxidation States

Oxidation states (or oxidation numbers) are assigned to elements in a compound to indicate their degree of oxidation or reduction. The oxidation state of an element can change during a chemical reaction, which is crucial for identifying redox processes. Common rules for determining oxidation states include that the oxidation state of an element in its elemental form is zero, and for monoatomic ions, it is equal to the charge of the ion.
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가이드 코스
02:42
Oxidation Numbers

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, reflecting the conservation of mass. In redox reactions, balancing often involves ensuring that both the number of electrons lost in oxidation and gained in reduction are equal. This process may require adjusting coefficients in front of compounds to achieve balance while maintaining the correct stoichiometry.
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01:32
Balancing Chemical Equations
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교과서 질문

Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) 2 AgNO3(aq) + CoCl2(aq) → 2 AgCl(s) + Co(NO3)2(aq)

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교과서 질문

Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) PBr3(l) + 3 H2O(l) → H3PO3(aq) + 3 HBr(aq)

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교과서 질문

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) I2O5(s) + 5 CO(g) → I2(s) + 5 CO2(g) (b) 2 Hg2+(aq) + N2H4(aq) → 2 Hg(l) + N2(g) + 4 H+(aq) (c) 3 H2S(aq) + 2 H+(aq) + 2 NO3-(aq) → 3 S(s) + 2 NO(g) + 4 H2O(l)

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교과서 질문

At 900 °C, titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction.

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교과서 질문

At 900 °C, titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride (c) Which substance is the reductant, and which is the oxidant?

교과서 질문

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) 2 MnO4-(aq) + 3 S2-(aq + 4 H2O(l) → 3 S(s) + 2 MnO2(s) + 8 OH-(aq) (b) 4 H2O2(aq) + Cl2O7(g) + 2 OH-(aq) → 2 ClO2-(aq) + 5 H2O(l) + 4 O2(g) (c) Ba2+(aq) + 2 OH-(aq) + H2O2(aq) + 2 ClO2(aq) → Ba(ClO2)2(s) + 2 H2O(l) + O2(g)

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