Find the charge in coulomb on 1 g-ion of N Exactly 0. The cathodic reactions in the cells are respectively. Calculate the volume of chlorine gas liberated at the electrode at NTP. Density of silver is Calculate the atomic mass of copper.
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These are homework exercises to accompany the Textmap created for "General Chemistry: Principles and Modern Applications " by Petrucci et al. Complementary General Chemistry question banks can be found for other Textmaps and can be accessed here. In addition to these publicly available questions, access to private problems bank for use in exams and homework is available to faculty only on an individual basis; please contact Delmar Larsen for an account with access permission. Chemical reactions can be used to produce electricity.
This electricity can be used in several different ways, and is applied in a variety of methods in our everyday lives. In studying theoretical cells and reactions, we can get a better understanding of the flow of electrons.
The following practice problems are to assist in your mastery of the topic of Electrochemistry. All reactants and products are in their standard states, and use data from the standard electrode reduction potentials table to predict whether the reaction is spontaneous in the forward reaction:.
For each of the following reactions below, draw a voltaic cell. In your drawing include the anode, cathode, and show the flow of electrons. Calculate the amount in grams of metal that is deposited at the cathode by running a current of 3. Assuming all reactants and products are currently in their standard states, determine which of the following reactions occur spontaneously and which can occur only through the use of electrolysis. Also, for those that require electrolysis, determine what the minimum voltage required is.
Since voltage is negative, it requires electrolysis with an applied voltage of greater than 1. This is a spontaneous reaction under standard conditions because it has positive V. Since the V is negative, it requires electrolysis with an applied V of greater than 0. After diluting the solution to The potential difference read 0. Therefore, Yes! Determine if these reactions are Endoenergonic or Exoenergonic under standard condition. Determine the anode and cathode of the following reactions.
Determine the voltage of the reactions below at non standard state. Given that an electrolysis process has taken place for 45 minutes and the grams of the lead being deposited was 3 g. What was the reading of the ammeter? Determine if these reactions are spontaneous or non spontaneous. Find a method to allow the non spontaneous reaction to take place. Therefore, the reaction is spontaneous.
For review on this topic, visit the page "Electrochemistry 1: Introduction". You may assume that the reactants and products in the equations are in their standard states. Use the information from Table P2 to predict if a spontaneous reaction will occur in the forward direction as drawn for the following cases.
Write the cell reactions for the electrochemical cells provided below. For review on this topic, visit the page "Electrochemistry 2: Galvanic cells and electrodes". For review on this topic, visit the page "Electrochemistry 3: Cell potentials and thermodynamics ".
This value is 0. Then plug in given values to the Nernst formula. For review on this topic, visit the page "Electrochemistry 4: The Nernst Equation ". Next, plug in the values given to the Nernst equation. The number of moles of electrons being transferred is 2. The equation will be set up as:. Set up the Nernst equation with the values appropriate for this equation. The moles of electrons transferred are 2. Solve for the value of x algebraically; this will yield an X value of 0.
Imagine an iron nail that is corroding in a solution. Predict the appearance of the nail under the given conditions using your knowledge of corrosion in voltaic cells. Assume standard temperature conditions. For review on this topic, visit the page " Electrochemistry 7: Electrochemical Corrosion ". Out of the reactions given below, which of the following can occur spontaneously only through electrolysis.
For those requiring electrolysis, what is the minimum voltage required? This means that we would need to apply a minimum of 1. For review on this topic, visit the page "Electrochemistry 8: Electrolytic cells and electrolysis". For review on this topic, visit the page "Electrochemistry 5: Applications of the Nernst Equation ". The moles of electrons transferred in the reaction is 2. A copper electrode was immersed in mL of water.
The potential was found to be 0. We use this concentration and account for the mass in grams. Given the following cell reaction, will the cell proceed spontaneously as written? Thus the ratio must be 2. For any additional information, consult "Electrochemistry". Spontaneous reaction at K. Non-spontaneous at K. Sketch a voltaic cell. Label anode and cathode. For voltaic cell, e - flow from anode to cathode. Salt bridge connects the two solutions.
The solution was then diluted to mL with water. Use the table of Standard Reduction Potential to predict whether these reactions will happen spontaneously.
Sketch a voltaic cell for each of the following conditions, labeling the anode, cathode, and electron flow. Balance the redox equation if necessary. Write and balance the net reaction using the two following half reactions. Find the Voltage for this reaction.
Need help? Visit the page "Cell Potential". Assuming all the reactants and products are in their standard state, use Table P2 to predict which reactions are spontaneous in the forward direction. In each of the following examples, write the cell diagram and cathode. Indicate the direction of the electron flow; write a balanced equation. Determine which half reaction is the cathode and the anode and calculate the reaction standard potential.
Determine whether a forward reaction is spontaneous or non-spontaneous:. What voltage is required for the electrolysis of the following reactions? All reactants are in standards states. Q22 For each of the following reactions below, draw a voltaic cell. Q59 By referring back to figure , explain what would happen at each individual circumstance zinc is wrapped around the head and tip of the iron nail a hole is poked at the center of an iron nail the nail is completely covered with copper S59 Through cathodic protection, zinc would get oxidized first.
The zinc would protect the nail from oxidation. Oxidation would occur even more because there would now be another head and tip. With more strained regions, the air would be able to oxidize the nail more.
The entire nail will be oxidized since copper isn't a sacrificial anode. It won't protect it from corrosion. Q63 Calculate the amount in grams of metal that is deposited at the cathode by running a current of 3.
Q65 Assuming all reactants and products are currently in their standard states, determine which of the following reactions occur spontaneously and which can occur only through the use of electrolysis.
Example Determine if the cell reaction for the following cell will proceed spontaneously in the forward direction. Is the cathode being diplaced in this reaction? Q2 Determine if these reactions are Endoenergonic or Exoenergonic under standard condition. Q5 Determine the anode and cathode of the following reactions. Q8 Determine the voltage of the reactions below at non standard state.
Q11 Explain What is corrosion? How corrosion occurs? How can corrosion be prevented? S11 Corrosion is a process whereby an element usually metal begins to degrade due to redox reaction.
It occurs due to the elements reaction with either oxygen gas, placing them in an acidic or basic solution.
6.9: Exercises on Electrochemistry