88.
Approximately what mass would be expected for a solution of Cd2+, if it were exposed for one minute to the same current and electrode used in the experiment?
C. A mass greater than 5.360 grams, but less than 6.182 grams
D. A mass greater than 6.182 grams
Highlight for correct answer: C
From passage,
A student sets up an experiment to determine the effects of the cell potential, concentration, and current on the degree of electroplating. In the first experiment, the student sets up six solutions with the following contents:
I: .1 M AgNO3 aq
II: 1.00 M AgNO3 aq
III: .1 M ZnSO4 aq
IV: 1.00 ZnSO4 aq
V: .1 M CuSO4 aq
VI: 1.00 M CuSO4 aq
Into each solution, an inert electrode weighing exactly 5grams is inserted. A steady current of electricity is applied to each electrode for the duration of one minute for all six solutions. The electrode is then removed and the mass is measured. The degree of plating can be determined by subtracting the original mass of the electrode from the final mass of the plated. electrode. The mass for each electrode after it is removed is listed below.
I: 6.187 grams
II: 6.182 grams
III: 5.360 grams
IV: 5.358 grams
V: 5.347 grams
VI: 5.350 grams
Answer Key: To form the same mass as the silver cation, cadmium would have to have twice the atomic mass of silver. (Why?) The atomic mass of cadmium (112g/m) is less than twice the atomic mass of silver (2 x 107 g/m), so the mass of Cd plated electrode muste be less than 6.182 grams (the mass of the lightest silver plated electrode).
Approximately what mass would be expected for a solution of Cd2+, if it were exposed for one minute to the same current and electrode used in the experiment?
C. A mass greater than 5.360 grams, but less than 6.182 grams
D. A mass greater than 6.182 grams
Highlight for correct answer: C
From passage,
A student sets up an experiment to determine the effects of the cell potential, concentration, and current on the degree of electroplating. In the first experiment, the student sets up six solutions with the following contents:
I: .1 M AgNO3 aq
II: 1.00 M AgNO3 aq
III: .1 M ZnSO4 aq
IV: 1.00 ZnSO4 aq
V: .1 M CuSO4 aq
VI: 1.00 M CuSO4 aq
Into each solution, an inert electrode weighing exactly 5grams is inserted. A steady current of electricity is applied to each electrode for the duration of one minute for all six solutions. The electrode is then removed and the mass is measured. The degree of plating can be determined by subtracting the original mass of the electrode from the final mass of the plated. electrode. The mass for each electrode after it is removed is listed below.
I: 6.187 grams
II: 6.182 grams
III: 5.360 grams
IV: 5.358 grams
V: 5.347 grams
VI: 5.350 grams
Answer Key: To form the same mass as the silver cation, cadmium would have to have twice the atomic mass of silver. (Why?) The atomic mass of cadmium (112g/m) is less than twice the atomic mass of silver (2 x 107 g/m), so the mass of Cd plated electrode muste be less than 6.182 grams (the mass of the lightest silver plated electrode).