(a)
Interpretation:
Whether the statement, “Silver metal is an electrode in the given cell reaction� is correct or not is to be identified.
(b)
Interpretation:
Whether the statement, “The aqueous solution of the given cell reaction contains
(c)
Interpretation:
Whether the statement. “No component is required in the given cell reaction� is correct or not is to be identified.
(d)
Interpretation:
Whether the statement, “The aqueous solution of the given cell reaction contains
(e)
Interpretation:
Whether the statement, “Cadmium metal is an electrode in the given cell reaction� is correct or not is to be identified.
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INTRODUCTION TO CHEMISTRY-ACCESS
- One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.0 M solution of Zn(NO3)2. A potential of 1.48 V is measured for this cell. Use this information to calculate the concentration of Ag+(aq).arrow_forwardOne half-cell in a voltaic cell is constructed from an iron electrode in an Fe(NO3)2 solution of unknown concentration. The other half-cell is a standard hydrogen electrode. A potential of 0.49 V is measured for this cell. Use this information to calculate the concentration of Fe2+(aq).arrow_forwardYou want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M)| Zn(s) half-cell is in one compartment. Identify several half-cells that you could use so that the cell potential will be close to (a) 1.1 V and (b) 0.50 V. Consider cells in which the zinc cell can be either the cathode or the anode.arrow_forward
- A voltaic cell is constructed using the reaction of chromium metal and iron(II) ions. 2 Cr(s) + 3 Fe2+(aq) 2 Cr3+(aq) + 3 Fe(s) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ________ half-cell to the ______ half-cell. The half-reaction at the anode is _______ and that at the cathode is ________.arrow_forwardA fuel cell designed to react grain alcohol with oxygen has the following net reaction: C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) The maximum work that 1 mole of alcohol can do is 1.32 103 kJ. What is the theoretical maximum voltage this cell can achieve at 25C?arrow_forwardConsider an electrochemical cell based on the half-reactions Ni2+(aq) + 2 e Ni(s) and Cd2+(aq) + 2e Cd(s). (a) Diagram the cell, and label each of the components (including the anode, cathode, and salt bridge). (b) Use the equations for the half-reactions to write a balanced, net ionic equation for the overall cell reaction. (c) What is the polarity of each electrode? (d) What is the value of Ecell? (e) In which direction do electrons flow in the external circuit? (f) Assume that a salt bridge containing NaNO3 connects the two half-cells. In which direction do the Na+(aq) ions move? In which direction do the NO3 (aq) ions move? (g) Calculate the equilibrium constant for the reaction. (h) If the concentration of Cd2+ is reduced to 0.010 M and [Ni2+] = 1.0 M, what is the value of Ecell? Is the net reaction still the reaction given in part (b)? (i) If 0.050 A is drawn from the battery, how long can it last if you begin with 1.0 L of each of the solutions and each was initially 1.0 M in dissolved species? Each electrode weighs 50.0 g in the beginning.arrow_forward
- Consider the following galvanic cell: Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is dead.arrow_forwardYou have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.arrow_forward
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