Question

4 4. a) Parts (a) through (c) below are all separate problems. A concentration cell, which is a type of voltaic cell, is set up with the following two half-cells: Half-cell #1 : Cu (s) electrode immersed in 1.00 L of 1.00 M Cu2+ (aq) Half-cell #2: Cu (s) electrode immersed in 1.00 L of 0.0010 M Cu2+ (aq) Answer the following questions about this concentration cell (1 pt each) i) What is the value of E° for this cell? Eo i) Which of the following is a correct statement about the voltage, E, for this cell? E>0 (circle) | E < 0 E=0 ii) Which half-cell is the anode in this concentration cell? (circle) | Half-cell #1 Half-cell #2 iv) If 1.00 L of water is added to Half-cell # 1, the cell voltage, E. will: (circle increase If 0.10 moles of Cu(NO3)2 (s) is dissolved in Half-cell #2, the cell voltage, E, will: (circle increase If 0.10 moles of NaCN (s) is dissolved in Half-cell #2, the cell voltage, E, will: (circle) increase decrease remain the same v) decrease remain the same vi) decrease remain the same b) For each of the following statements, circle True or False to indicate whether or not the statement is correct. (2 pts each) i) True False The absolute entropy of a substance increases as temperature increases. ii) True False A reaction must be spontaneous if entropy of the reaction is increasing. iii) True False If ΔΗΡ > 0 and AS° < 0 for a particular reaction, then the reaction will be nonspontaneous at standard states at all temperatures.