Equations 1. CaCO3(s) CaO(s) + CO₂(g) 2. SO₂(g) + NO₂(g) → SO3(g) + NO(g) - 3. H₂O(l) + Cl₂O(g) → 2HOCI(g) 4. C6H₁2O6(S) - CO₂(g) + C₂H5OH(1) 5. SO₂(g) + H₂O(l) → H₂SO3(aq) 6. 2HNO3(aq) → N₂O5(g) + H₂O(l) 7. NaOH(aq) + Al(s) + H₂O(l) 8. 2NH3(aq) + NaOCI(aq) → N₂H4(aq) + NaCl(aq) + H₂O(1) +1 -1 2H₂O2(1) → Examine the above equations numbered 1-8. Identify which equations are examples of redox reactions and list the equation numbers in ascending numerical order. + + + Select one: O N₂O4(9) - Which of the following equations is an example of disproportionation? H₂(g) + NaAlO₂ (s) +1 -2 0 2H₂O(1) + O2(g) 2NO₂(g) 20F₂(g) → 2F₂(g) + O₂(g) NH4Cl(s) HCI(g) + NH3(g) 2H₂O₂(1)→ 2H₂O(l) + O₂(g) The oxidation number of an element changes from +4 to -2. Therefore, the element was acting as a ◆ agent by electrons.
Equations 1. CaCO3(s) CaO(s) + CO₂(g) 2. SO₂(g) + NO₂(g) → SO3(g) + NO(g) - 3. H₂O(l) + Cl₂O(g) → 2HOCI(g) 4. C6H₁2O6(S) - CO₂(g) + C₂H5OH(1) 5. SO₂(g) + H₂O(l) → H₂SO3(aq) 6. 2HNO3(aq) → N₂O5(g) + H₂O(l) 7. NaOH(aq) + Al(s) + H₂O(l) 8. 2NH3(aq) + NaOCI(aq) → N₂H4(aq) + NaCl(aq) + H₂O(1) +1 -1 2H₂O2(1) → Examine the above equations numbered 1-8. Identify which equations are examples of redox reactions and list the equation numbers in ascending numerical order. + + + Select one: O N₂O4(9) - Which of the following equations is an example of disproportionation? H₂(g) + NaAlO₂ (s) +1 -2 0 2H₂O(1) + O2(g) 2NO₂(g) 20F₂(g) → 2F₂(g) + O₂(g) NH4Cl(s) HCI(g) + NH3(g) 2H₂O₂(1)→ 2H₂O(l) + O₂(g) The oxidation number of an element changes from +4 to -2. Therefore, the element was acting as a ◆ agent by electrons.
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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Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:Equations
1. CaCO3(s) CaO(s) + CO₂(g)
2. SO₂(g) + NO₂(g) → SO3(g) + NO(g)
3. H₂O(1) + Cl₂O(g) → 2HOCI(g)
4. C6H12O6(S) - CO₂(g) + C₂H₂OH(1)
5. SO₂(g) + H₂O(l) → H₂SO3(aq)
6. 2HNO3(aq) → N₂O5(9) + H₂O(1)
7. NaOH(aq) + Al(s) + H₂O(l) → H₂(g) + NaAlO₂ (s)
8. 2NH3(aq) + NaOCI(aq) → N₂H4(aq) + NaCl(aq) + H₂O(l)
Examine the above equations numbered 1-8. Identify which equations are examples of redox reactions and list the equation numbers in ascending numerical order.
Which of the following equations is an example of disproportionation?
+1 -1
+1 -2
0
2H₂O2(1)→ 2H₂O(1) + O₂(g)
Select one:
N₂O4(9) 2NO₂(g)
20F₂(g) → 2F₂(g) + O₂(g)
NH4Cl(s) → HCI(g) + NH3(g)
2H₂O₂(1)→ 2H₂O(l) + O₂(g)
The oxidation number of an element changes from +4 to -2. Therefore, the element was acting as a
+ agent by
electrons.
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