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Balanced equation: Oxidizing agent: Reducing agent:

Balanced equation: Oxidizing agent: Reducing agent:

Chemistry
Chemistry
10th Edition
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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2. KMNO4 + NagC204 + H2SO4 K2SO4 + MNSO4 + NagSO4 + CO2+ H20 Balanced equation: Oxidizing agent: Reducing agent: Criteria for each item Solution following the 5-step process Balanced equation Oxidizing agent Reducing agent 10 points 3 points 1 point 1 point Total points or each item: 15points
Transcribed Image Text:2. KMNO4 + NagC204 + H2SO4 K2SO4 + MNSO4 + NagSO4 + CO2+ H20 Balanced equation: Oxidizing agent: Reducing agent: Criteria for each item Solution following the 5-step process Balanced equation Oxidizing agent Reducing agent 10 points 3 points 1 point 1 point Total points or each item: 15points
DISCOAEK Step 1: Assign the oxidation numbers of the elements in the chemical equation, FepO3(s) + CO(g) – Fe(s) + CO2lg) +2 -2 Oxidation numbers: +3 -2 +4 -2 Step 2: Determine which elements undergo changes in oxidation state. There are two elements that undergo changes in oxidation state, C and Fe. Step 3: Determine the total increase and decrease in oxidation number or total number of electrons lost and gained. From C42 to C+, oxidation number increaed by 2 per C or 2 electrons lost. From Fe+3 to Fe", oxidation number decreased by 3 per Fe, but since there are 2Fe involved, indicated by the subscript of Fe, total decrease is 2 x 3 = 6 or 6 electrons gained. olgmx +2 Fo) + đở) - Fe(s) + to ) dosle or E Sups ai coi i Btep 4: Equalize the increase and decrease in oxidation number or total electrons lost and gained by figuring out the proper multiplier which will become the new coefficients in the chemical equation. For the sample equation, equalize electrons lost and 3 electrons gained. To do this, multiply by the lowest possible integers or multipliers that will gve the same product. The multipliers become the coefficients. +3 -2 Fel»)+CO 3 x2=-6 Step 5: Finish balancing by counting the number of atoms of each elemnt then adjusting the coefficients until the same number of atoms are found on both sides of the equation. Usually oxygen is counted last. The balanced equation is, Balanced equation : Fe2Oa(s)+3CO(g)→2FE(s)+3CO2{g)
Transcribed Image Text:DISCOAEK Step 1: Assign the oxidation numbers of the elements in the chemical equation, FepO3(s) + CO(g) – Fe(s) + CO2lg) +2 -2 Oxidation numbers: +3 -2 +4 -2 Step 2: Determine which elements undergo changes in oxidation state. There are two elements that undergo changes in oxidation state, C and Fe. Step 3: Determine the total increase and decrease in oxidation number or total number of electrons lost and gained. From C42 to C+, oxidation number increaed by 2 per C or 2 electrons lost. From Fe+3 to Fe", oxidation number decreased by 3 per Fe, but since there are 2Fe involved, indicated by the subscript of Fe, total decrease is 2 x 3 = 6 or 6 electrons gained. olgmx +2 Fo) + đở) - Fe(s) + to ) dosle or E Sups ai coi i Btep 4: Equalize the increase and decrease in oxidation number or total electrons lost and gained by figuring out the proper multiplier which will become the new coefficients in the chemical equation. For the sample equation, equalize electrons lost and 3 electrons gained. To do this, multiply by the lowest possible integers or multipliers that will gve the same product. The multipliers become the coefficients. +3 -2 Fel»)+CO 3 x2=-6 Step 5: Finish balancing by counting the number of atoms of each elemnt then adjusting the coefficients until the same number of atoms are found on both sides of the equation. Usually oxygen is counted last. The balanced equation is, Balanced equation : Fe2Oa(s)+3CO(g)→2FE(s)+3CO2{g)
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