Sample of solid aluminum (Al) and solid magnesium (Mg) are placed in a solution containing 1.0 M Al3+ ion and 1.0 M Mg2+ ions at 25 o C. For the mixture…
(1) write the BALANCED spontaneous reaction,
(2) determine the cell potential (Ecell) in volts,
(3) the free energy (ΔG) in kJ, and
(4) the equilibrium constant (Keq).
Al3+ (aq) + 3 e– "Al (s) Eo = –1.66 V
Mg2+ (aq) + 2 e– "Mg (s) Eo = –2.37 V
Sample of solid aluminum (Al) and solid magnesium (Mg) are placed in a solution containing 1.0...
When solid magnesium is reacted with an aluminum phosphate solution, metallic aluminum is produced by single displacement (equation. a): (a) AlPO4(aq)+Mg(s)→Al(s)+Mg3(PO4)2(aq) Balance equation (a) and answer the following: How many grams of aluminum metal should be theoretically produced from 2.338 g of pure magnesium metal. Suposse magnesium metal is the limiting reactant. Molar masses (g/mol): AlPO4 = 121.95 Mg = 24.305 Al = 26.98 Mg3(PO4)2 = 262.86 Important note: Use 3 digits after the decimal place in your answer.
Magnesium ions and sulfate ions have the following reduction and oxidation reactions and potentials: Mg2+(aq) + 2e– →Mg(s) Eo = –1.18 V 2SO42–(aq)→S2O82–(aq) + 2e– Eo = –2.05 V Why did neither of these half-reactions occur when the magnesium sulfate solution was electrolyzed?
Calculate the theoretical cell potential (E°) of a galvanic cell under standard conditions made up of copper and magnesium (see Part II and Table 1 for more information). PARTIL Creating and Testing Voltaic Cells Introduction and Background for the Voltaic Cells A galvanic cell (sometimes more appropriately called a voltaic cell) consists of two half-cells joined by a salt bridge that allow ions to pass between the two sides in order to maintain electroneutrality. Each half-cell contains the Components of...
20. A galvanic (voltaic) cell is constructed froma half-cell containing a solid aluminum electrode dipped in a 1.0 M Al(NO3)3 solution and a half-cell containing a solid indium electrode in contact with a 1.0 M In(NO3)3 solution. The half-cells are linked by an external circuit (a wire) and by a KCl salt bridge. The cell generates a standard voltage of 1.32 V and the indium electrode is positive. The standard half-cell reduction potential for aluminum, E°(Al3*/Al), is listed in the...
8. (2 pts) Use the tabulated half-cell potentials to calculate AGⓇ for the following balanced redox reaction. 3 Mg2+(aq) + 2 Al(s) 3 Mgs) + 2 A13+(aq) E° Mg2(aq) + 2e → Mg(s) R -2.37 V AP (aq) + 3e + Al(s) O -1.66 V Cathode Anode a. - 2.3 x 10² kJ b. +4.1 x 102 kJ c. +1.4 x 10² kJ d. - 7.8 x 10 kJ
Given: 3Mg(s) +2 A13+(aq) – 2 Al(s) + 3Mg2+(aq) Which of the foloowing statements is/are correct? a. Mg metal is oxidized and Aluminum ion is reduced b. Mg metal is reduced and Aluminum ion is oxidized C. Aluminum metal is oxidized and Magnesium metal is reduced d. Aluminum metal is reduced and Magnesium ion is oxidized e. None of the these is correct Use the standard half-cell potentials listed below to calculate the standard cell potential and standard free energy...
7.An electrochemical cell consists of a Mg electrode in a solution of 0.548 M Mg+ coupled to a Pd electrode in a solution of 0.438 M Pd2+ , all held at 20.1 °C. Mg+(aq) + e− ⇌ Mg(s) E° = -2.700 V Pd2+(aq) + 2e− ⇌ Pd(s) E° = 0.951 V 1. Determine Ecell (in V). Report your answer to three decimal places in standard notation (i.e. 1.234 V). Tries 0/3 2. Determine ΔG (in kJ). Report your answer to three significant...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
question 1 & 2 1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCI was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of...
1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - Keq <1 E° - ΔG° - Keq <1 E° + ΔG°+ Keq >1 E° + ΔG°- Keq >1 E° - ΔG° + Keq <1 2. What information can be obtained from the Figure below? The equivalence point occurs at pH = 7.0 but the pKa is not known from the graph. Both the pOH and the...