Electrolysis is the process of using electrical current to cause a nonspontaneous reaction to occur. For example, water molecules do not readily decompose into hydrogen and oxygen. However, water can be decomposed using electrolysis according to the reaction 2 H₂O(1)→ 2H₂(g) + O₂(g) Because electrolysis involves the transfer of electrons, it is classified as a type of oxidation-reduction (redox) reaction. For the given reaction, identify which atoms are oxidized and which are reduced. Which atoms are oxidized? Both oxygen atoms in O₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂(g). Both hydrogen atoms in H₂O(1). MacBook Pro Which atoms are reduced? Both hydrogen atoms in H₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂O(1). Both oxygen atoms in O₂(g).

Electrolysis is the process of using electrical current to cause a nonspontaneous reaction to occur. For example, water molecules do not readily decompose into hydrogen and oxygen. However, water can be decomposed using electrolysis according to the reaction 2 H₂O(1)→ 2H₂(g) + O₂(g) Because electrolysis involves the transfer of electrons, it is classified as a type of oxidation-reduction (redox) reaction. For the given reaction, identify which atoms are oxidized and which are reduced. Which atoms are oxidized? Both oxygen atoms in O₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂(g). Both hydrogen atoms in H₂O(1). MacBook Pro Which atoms are reduced? Both hydrogen atoms in H₂(g). The oxygen atom in H₂O(1). Both hydrogen atoms in H₂O(1). Both oxygen atoms in O₂(g).

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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+ |I P. ト [Review Topics] [References] Iron metal is obtained by reduction of iron(III) oxide with powdered aluminum. The reaction is highly exothermic, and the products are molten AlO3 (1) and Fe(l). Write the balanced equation for this reduction. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) Retry Entire Group 8 more group attempts remaining Submit Answer Previous Next Save and Exit NOV 1 étv 14 MacBook Air 000 000 DD F12 F10 F7 6 F4 F5 ) ( %24 dele 8. 6. 9 { [ R } %3D
Balance the following redox reactions that occur under acidic conditions. 2. MnO4-1 (aq) + H2O2 (aq) Mn+2 (aq) + O2 (g) 3. CrO4-2 (aq) + N2O (g) Cr+3 (aq) + NO (g) 4. HCOOH (aq)+ MnO4- (aq) CO2 (g) + Mn+2 (aq)
4. During space travel, oxygen O₂ is used for astronauts' breathing and as a fuel. It is constantly being produced onboard space crafts using water H₂O as the reactant in the following electrolysis reaction: 2H₂O (1)→ 2H2(g) + O₂(g) The two key half reactions are listed below as their reduction reactions: 2H₂O(1) +2e → H₂(g) + 2OH(aq) 2H₂O(1) + O₂(g) + 4c →40H (aq) a. What is the minimum potential to drive this reaction? b. A battery providing a constant current of 3.00 A is used for this electrolytic cell in the generation of O₂. What is the mass of Oz (in g) that is produced after running the battery for 1 hour? Use 32.0 g/mol for the molar mass of 0₂.
Balance the following reaction in acidic solution. Cr₂O²(aq) + HNO₂ (aq) → Cr³+ (aq) + NO3(aq) - Fill in the coefficients for the balanced overall equation. HNO₂ + H+ + Cr₂0,²- NO + 2 Cr3+ + H₂O O
For each reaction, write the chemical formulae of the oxidized reactants in the space provided. Write the chemical formulae of the reduced reactants in the space provided. reactants oxidized: 2 AgNO, (aq) + Mg(s) → 2Ag(s) + : Mg(NO,), (aq) 2 reactants reduced: reactants oxidized: Feso, (ag) + Mg(s) → Fe(s) + MgS0,(aq) reactants reduced: reactants oxidized: Ca (s) + ZnCl, (aq) → Zn (s) + CaCl, (a q) reactants reduced:
In an basic solution, permanganate ion, MnO₄⁻ , reacts with Sn(II) ion to give Mn(II) ion and Sn(IV) ion: MnO₄⁻ + Sn²⁺ → Mn²⁺ + Sn⁴⁺ Complete and balance the following redox equation using the set of smallest whole-number coefficients. Now sum the coefficients of all species in the balanced equation. (Remember the coefficients that are equal to one.) The sum of the coefficients is: A) 28 B) 35 C) 38 D) 42 E) 30
Balancing the following redox reaction that occurs in an acid medium, it is found that the coefficients Cl + and H + are:
Consider the following equation in aqueous solution: Cr:0,2 (aq) + S2O3² (aq) → Cr®*(aq) + S.O² (aq) Given that sulfur is oxidized, write the half-reaction for the oxidation in acidic solution. S:0:2-(aq) → S.Oc²-(aq) D2+|03+ 74+ 1 3 5 7 8 9 04 18 Do 5 (s) (1) (g) (aq) + H2O e H+ H H3O+ Reset • x H2O Delete 1L 4.
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Report all answers with the proper number of significant figures. In an electrolysis experiment similar to the one employed this experiment; a student observed that his unknown metal anode lost 0.238 grams while a total volume of 94.50 mL of hydrogen was being produced. The temperature of the solution was 25°C and the barometric pressure was 739 mm Hg. The difference between the water levels in the beaker and buret was negligible. The vapor pressure of water at 25°C is 23.8 mm Hg. Based on the information provided and the lab handout, what pressure of hydrogen is collected, in atmospheres? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer units