In a voltaic cell, oxidation occurs at the Positive terminal cathode terminal anode terminal What is...
Determine whether each statement describes an anode or a cathode in a voltaic cell. Where the reduction occurs Choose... The positive terminal Choose... Where electrons flow from Choose... Where the oxidation occurs Choose... Where electrons flow to Choose... The negative terminal Choose...
Item 5 Part A What reaction (oxidation or reduction) occurs at the cathode of a voltaic cell? O reduction oxidation Submit Request Answer Part B What is the sign of the cathode? O O positive (+) negative (-) Submit Request Answer Part Do electrons flow toward or away from the cathode? O flow toward flow away
Item 4 Part A What reaction (oxidation or reduction) occurs at the anode of a voltaic cell O reduction O oxidation Submit Request Answer Part B What is the sign of the anode? o negative (-) positive (+) Submit Request Answer Part Do electrons flow toward or away from the anode? flow toward flow away
Draw a voltaic pile, or “crown of cups.” Label the anode (+ terminal) and the cathode (- terminal), and the electrolyte. Give examples of what each of these substances might be.
Part A Consider a voltaic cell that is set up as follows: Anode contains an Zn(s) electrode and 1M Zn2+(aq) Cathode contains a Pt(s) electrode and 1M MnO4–(aq),Mn2+(aq), and H+(aq) Which of the following statements match the cathode? Select all that apply. Group of answer choices The electrode increases in mass Oxidation occurs at this half-cell Electrons enter the half-cell The electrode is inactive Cations from the salt-bridge move to this half-cell The electrode is negative Part B Which of...
QUESTION 10 Which of the following statements concerning a voltaic cell is FALSE? A voltaic cell uses an oxidation-reduction reaction to produce electrical energy. O The oxidation half reaction occurs at the cathode. O The cell consists of two half cells. O At the anode a substance will lose electrons. O The anode and the cathode are separated by a salt bridge.
Determine which of the following is True about what occurs at the anode of any voltaic cell. 1) Electrons enter the anode through the external circuit. ["True", "False"] 2) The mass (in grams) of the anode decreases as the reaction occurs (assuming that the anode is a reactant). ["False", "True"] 3) A substance undergoes oxidation. ["False", "True"]
5. A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver (I) ions. Solutions of 1.00 M silver nitrate and zinc nitrate also were used. The anode is on the left, the cathode is on the right. Where does oxidation occur? 5. A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver (I) ions. Solutions of 1.00 M silver nitrate and zinc nitrate also were used....
A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.700 M and 0.120 M , respectively. The volume of half-cells is the same. Question 2 1 pts A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25°C. The initial concentrations of Ni2+ and Zn2+ are 1.700 M and 0.120 M, respectively. The volume of half-cells is the same. What is the concentration...
A voltaic cell is constructed in which the anode is a Ag Ag half cell and the cathode is a CI Cl2 half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: the Ag Ag electrode. |the CIICl2 electrode In...