What is the free energy change in kJ for the reaction below? 2 ClO3−(aq) + 12 H+(aq) + 5 Co(s) → Cl2(g) + 6 H2O(l) + 5 Co2+(aq)

What is E°cell for the following reaction? Is this reaction spontaneous under standard conditions? Cu2+(aq) + Sn2+(aq) → Cu(s) + Sn4+(aq) Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V Group of answer choices –0.21 V, nonspontaneous 0.21 V, spontaneous 0.21 V, nonspontaneous –0.21 V, spontaneous

The standard EMF for the cell using the overall cell reaction below is +0.84 V: 2Al(s) + 312 (s) 2A1³+ (aq) + 61 (aq) What is AGO for the cell reaction in kJ? Express your answer in decimal notation to one decimal place, without units.

Calculate AG for the following reaction at 25 °C: rxn H₂O2(g) → H₂O₂ (1)

Qd 125.

A certain metal M forms a soluble nitrate salt M(NO3)3. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M(NO3)3 and the right half cell with a 10.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 20.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 0 ○ left ☐ x10 O right ×

6. Eqn 1: ZnS(s) Eqn 2: S(s) + O2(g) →SO2(g) Eqn 3: ZnS(s) + O2(g)→ Zn(s) + SO>(g) → Zn(s) + S(s) AG° = +198.3 kJ AG° =-300.1 kJ The decomposition of zinc sulfide (represented by Equation 1) can be accomplished by coupling the reaction to the combustion of sulfur (represented in Equation 2), which results in the overall reaction represented in Equation 3. a. Determine the free energy change for the reaction represented in Equation 3. b. Explain why the reactions represented in Equations 1 and 2 are suitable for coupling to produce a thermodynamically favorable process.

When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced net equation for the reaction. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) Help chemPad XXº → Greek How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCI? kJ How can you harness this reaction to do useful work? This is accomplished by making ---Select--- produce a voltage. cell that ---Select--- the reduction reaction and the oxidation reaction in order to control the flow of ---Select--- through a wire to