Use date from Table 19.1 to predict whether, to any significant extent,
a. Mg(s) will displace
b. Sn(s) will react with and dissolve in 1 M HCl;
c.
d.
e.
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General Chemistry: Principles and Modern Applications (11th Edition)
- An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forwardA constant current of 1.25 amp is passed through an electrolytic cell containing a 0.050 M solution of CuSO4 and a copper anode and a platinum cathode until 3.00 g of copper is deposited. a How long does the current flow to obtain this deposit? b What mass of silver would be deposited in a similar cell containing 0.15 M Ag+ if the same amount of current were used?arrow_forwardUse Table 17.1 to predict what reaction, if any, will occur if sulfur is added to acidic aqueous solutions of the following species at standard conditions. (a) MgBr2 (b) Sn(NO3)2(c) Cr(ClO3)2arrow_forward
- A constant current of 1.40 amp is passed through an electrolytic cell containing a 0.100 M solution of AgNO3 and a silver anode and a platinum cathode until 2.48 g of silver is deposited. a How long does the current flow to obtain this deposit? b What mass of chromium would be deposited in a similar cell containing 0.100 M Cr3+ if the same amount of current were used?arrow_forwardAn electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forwardAn electrochemical cell is made by placing an iron electrode in 1.00 L of 0.15 M FeSO4 solution and a copper electrode in 1.00 L of 0.040 M CuSO4 solution. a What is the initial voltage of this cell when it is properly constructed? b Calculate the final concentration of Cu2+ in this cell if it is allowed to produce an average current of l.25 amp for 375 s.arrow_forward
- Use Table 17.1 to select (a) a reducing agent in acidic solution that converts ClO3- to Cl2 but not Cr2O72- to Cr3+. (b) an oxidizing agent that converts Mg to Mg2+ but not Mn to Mn2+. (c) a reducing agent in basic solution that converts NO2- to NO3- but not OH- to O2.arrow_forwardCalculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)arrow_forwardAn electrode is prepared by dipping a silver strip into a solution saturated with silver thiocyanate, AgSCN, and containing 0.10 M SCN . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.45 V. What is the solubility product of silver thiocyanate?arrow_forward
- In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?arrow_forwardA galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forwardOrder the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ).arrow_forward
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