Can someone explain this question for me?
I understand I have to find an action potential, Q value and use a Nernst equation, but I can not actually apply those into a question.
Thanks
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Can someone explain this question for me?
I understand I have to find an action potential,...
Can someone please tell me if I did the equations right and if the anode and...
Can someone please tell me if I did the equations right and if the
anode and cathode reactions are correct .
Report sheet Exp. 11 Electrochemistry Date: Name: Partner's Name: Lab Section Anode Equation for the Cathode Equation for the Cathode Cell Ecell Reaction Anode Reaction oxidahon) Measured Cu-Zn MO Cu-Fe Zn-Mg M9 Fe-Mg Mg 2n
This is the third time I've posted this question. Can someone please help me with the...
This is the third time I've
posted this question. Can someone please help me with the top one.
I slipped in a similar example. And the answer is not 2.4135
Consider the following cell reaction Fe(s)2 H ? M)-Fe2(100 M) +H>(g\1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH Consider the following cell reaction Ni(s)2 H (? M) Ni(100 M)Hg100 atm) If the cell potential at 298 K...
Could someone help me? I slipped in a previous example for reference Consider the following cell...
Could someone help me? I
slipped in a previous example for reference
Consider the following cell reaction: Fe(s) + 2 H+(?M —Fe2+(1.00 M)+H gX1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH= Consider the following cell reaction: Ni(s) + 2 H (?M) —+NI+(1.00 M)+H(E)1.00 atm) If the cell potential at 298 K is 0.104 volts, what is the pH of the hydrogen electrode? pH - 1.75 x Incorrect...
This is all the information I was given to answer this question. To determine the formation...
This is all the information I was given to answer this
question.
To determine the formation constant, Kf, for [Zn(CN)4)2-(aq), 4.00 mL of 1.50 mol/L KCN(aq) and 1.00 mL of 0.0750 mol/L Zn(NO3)2(aq) were combined. The mixture was stirred for 10 minutes to ensure that equilibrium had been reached. A voltaic cell was constructed to determine the concentration of uncomplexed Zn2+ (aq) ions left in solution at the end of the complexation reaction. The [Zn(CN)4]- (aq), Zn2+ (aq), CN (aq)...
Can someone please help me out with this problem? If possible could you add steps so...
Can someone please help me out
with this problem? If possible could you add steps so that I can be
able to do the rest on my own? Thank YOUUUU!!
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N (9)+4H2O(1)+4e → N H (aq)+4 OH (aq) Ered = -1.16 V Zn²+ (aq)+2e → Zn(s) Exped=-0.763 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at...
how would you go about solving this problem via using equations just looking for the equation order i should go about solving this problem In this experiment you will be using the two half rea...
how
would you go about solving this problem via using equations
just looking for the equation order i should go about solving this
problem
In this experiment you will be using the two half reactions Cu?"/Cu and Zn2 /Zn. The standard electrode potential, E°, for these half reactions is +0.34V and-0.76V respectively, so the Nernst Equation for these half reactions is the following Cu ea)+2e - Cus) E - 0.34V 0.0592V Cu2+] 0.0592V Zn 2 Note that solids by definition...
Can someone please help me answering this question part a and b. 3. The value of...
Can
someone please help me answering this question part a and b.
3. The value of E' for the following reaction is 0.189 V. a. What is the value of Ece given the concentrations shown? 4H) + Fe(s) + NO, 10) ► Fel) + NO + 2 H20 H: 0.1 M, NO,: 0.6 M, Fel: 1.0 M, NO: 0.5 M b. Draw a diagram of the cell, indicating the anode, cathode and electron flow through the salt bridge.
Chem 1212 Lab Report on electrochemistry Electrochemistry When electrons transfer between reaction components in a redox...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
please solve all correctly Question: Consider the voltaic cell using silver and zinc. The net equation...
please solve all correctly
Question: Consider the voltaic cell using silver and zinc. The net equation for this voltaic cell is 2Ag+ (aq) + Zn(s)--> 2Ag(s) + Zn2+lag) Calculate the molar concentration of Ag+ if a potential of 1.58 V was measured across the cell when the molar concentration of Zn* was 0.150 M. Hint: You need to first calculate the of the cell. Given the following Data: Be sure to show all calculations Half-Reaction Standard Potential E* (volts) Ag...
Can someone explain Carbonate for me? CO3 what I don't understand: visualizing the loss of electrons,...
Can someone explain Carbonate for me? CO3 what I don't understand: visualizing the loss of electrons, when I see other ionic compounds like PO4 I just count backwards along the periodic table to account for the charges of the oxygen atoms, yet when I attempt to do that with C, you end up in the grey area of the periodic table where no element exists (the d block next to the He atom). Furthermore since Carbon loses all of its...
Can someone please tell me if I did the equations right and if the
anode and cathode reactions are correct .
Report sheet Exp. 11 Electrochemistry Date: Name: Partner's Name: Lab Section Anode Equation for the Cathode Equation for the Cathode Cell Ecell Reaction Anode Reaction oxidahon) Measured Cu-Zn MO Cu-Fe Zn-Mg M9 Fe-Mg Mg 2n
This is the third time I've
posted this question. Can someone please help me with the top one.
I slipped in a similar example. And the answer is not 2.4135
Consider the following cell reaction Fe(s)2 H ? M)-Fe2(100 M) +H>(g\1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH Consider the following cell reaction Ni(s)2 H (? M) Ni(100 M)Hg100 atm) If the cell potential at 298 K...
Could someone help me? I
slipped in a previous example for reference
Consider the following cell reaction: Fe(s) + 2 H+(?M —Fe2+(1.00 M)+H gX1.00 atm) If the cell potential at 298 K is 0.307 volts, what is the pH of the hydrogen electrode? pH= Consider the following cell reaction: Ni(s) + 2 H (?M) —+NI+(1.00 M)+H(E)1.00 atm) If the cell potential at 298 K is 0.104 volts, what is the pH of the hydrogen electrode? pH - 1.75 x Incorrect...
This is all the information I was given to answer this
question.
To determine the formation constant, Kf, for [Zn(CN)4)2-(aq), 4.00 mL of 1.50 mol/L KCN(aq) and 1.00 mL of 0.0750 mol/L Zn(NO3)2(aq) were combined. The mixture was stirred for 10 minutes to ensure that equilibrium had been reached. A voltaic cell was constructed to determine the concentration of uncomplexed Zn2+ (aq) ions left in solution at the end of the complexation reaction. The [Zn(CN)4]- (aq), Zn2+ (aq), CN (aq)...
Can someone please help me out
with this problem? If possible could you add steps so that I can be
able to do the rest on my own? Thank YOUUUU!!
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N (9)+4H2O(1)+4e → N H (aq)+4 OH (aq) Ered = -1.16 V Zn²+ (aq)+2e → Zn(s) Exped=-0.763 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at...
how
would you go about solving this problem via using equations
just looking for the equation order i should go about solving this
problem
In this experiment you will be using the two half reactions Cu?"/Cu and Zn2 /Zn. The standard electrode potential, E°, for these half reactions is +0.34V and-0.76V respectively, so the Nernst Equation for these half reactions is the following Cu ea)+2e - Cus) E - 0.34V 0.0592V Cu2+] 0.0592V Zn 2 Note that solids by definition...
Can
someone please help me answering this question part a and b.
3. The value of E' for the following reaction is 0.189 V. a. What is the value of Ece given the concentrations shown? 4H) + Fe(s) + NO, 10) ► Fel) + NO + 2 H20 H: 0.1 M, NO,: 0.6 M, Fel: 1.0 M, NO: 0.5 M b. Draw a diagram of the cell, indicating the anode, cathode and electron flow through the salt bridge.
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
please solve all correctly
Question: Consider the voltaic cell using silver and zinc. The net equation for this voltaic cell is 2Ag+ (aq) + Zn(s)--> 2Ag(s) + Zn2+lag) Calculate the molar concentration of Ag+ if a potential of 1.58 V was measured across the cell when the molar concentration of Zn* was 0.150 M. Hint: You need to first calculate the of the cell. Given the following Data: Be sure to show all calculations Half-Reaction Standard Potential E* (volts) Ag...
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