Question
In: Chemistry
A magnesium electrode in 1 M MgSO4 and an iron electrode in 1 M FeSO4 are...
A magnesium electrode in 1 M MgSO4 and an iron electrode in 1 M FeSO4 are in electrical contact forming a galvanic cell. Determine the direction the electrons flow, write the reaction that occurs at the cathode and the reaction that occurs at the anode and finally determine the total emf for the reaction.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and a copper electrode...
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and
a copper electrode in 1 M Cu(NO3)2. What is the equilibrium
constant for this reaction at 25oC? Enter you answer with 2
significant digits, using the syntax of "1.0x10(22)" for
"1.0x1022"
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and a copper electrode...
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and
a copper electrode in 1 M Cu(NO3)2. What is the equilibrium
constant for this reaction at 25oC? Enter you answer with 2
significant digits, using the syntax of "1.0x10(22)" for
"1.0x1022
What is the cell potential (emf, in V) of this cell at
25oC?
Cu |Cu2+ (0.0510 M) ‖ Br2 |Br-
(0.363 M)
What mass (in g) of aluminum can be electroplated when 0.855
amps are used...
Magnesium reacts with iron (II) Chloride to form magnesium chloride and iron. A mixture of 41.0g...
Magnesium reacts with iron (II) Chloride to form magnesium
chloride and iron. A mixture of 41.0g of magnesium and 175 g of
iron (II) chloride is allowed to react. Identify the limiting
reactant and determine the mass of the excess reactant.
An electrochemical cell, composed of an iron electrode (anode) immersed in 0.10 M Fe (NO3)2 and...
An electrochemical cell, composed of an iron electrode (anode)
immersed in 0.10 M Fe (NO3)2 and silver electrode (cathode)
immersed in 0.11M AgNO3, was found to have a cell potential of
1.21V. The standard reduction potential for Ag+ / Ag half-cell is
+0.80V. The standard reduction potential for the Fe+2/ Fe half –
cell is -0.45V.
1. Write the half-cell reaction at the anode.
2.Write the half –cell reaction at the Cathode
3.Write over all cell
reaction
4. Determine the...
You mix 25.0ml of 6.0m LiOH with 75.0ml of MgSO4. Magnesium hydroxide precipitates from the solution....
You mix 25.0ml of 6.0m LiOH with 75.0ml of MgSO4. Magnesium
hydroxide precipitates from the solution.
A. Write a balanced equation for the reaction.
B. What concentration of MgSO4 is required to react with all the
LiOH?
C. What mass of magnesium hydroxide is produced?
D. What is the final concentration of Li2SO4(aq)?
Which of these metals does not act as a sacrificial electrode for iron?
Which of these metals does not act as a sacrificial electrode
for iron?MgMn ZnCu
Consider Galvanic cell consisting of a Mg electrode immersed in a solution of magnesium nitrate and...
Consider Galvanic cell consisting of a Mg electrode immersed in
a solution of magnesium nitrate and a silver electrode immerse in a
solution of silver nitrate. Knowing that Mg2++2e—>Mg(s) -2.37V;
and Ag+e—> Ag(s). +8.0V
A)what value of the reaction quotient could trigger a change in the
spontaneity of the reaction?
B)If the [Mg2+]was equal to 1.0*10^-10M for the value of the
reaction quotient In A), what would be the [Ag+]?
Sketch and briefly explain a cell composed of 1 M CuSO4, Cu electrode and 1 M...
Sketch and briefly explain a cell composed of 1 M CuSO4, Cu
electrode and 1 M ZnSO4 and a Zn electrode, Calculate the Emf and
don’t forget to show the salt bridge.
Iron(II) Sulfate forms a blue-green hydrate with the formula FeSO4 ·n H2O(s). If this hydrate is...
Iron(II) Sulfate forms a blue-green hydrate with the formula
FeSO4 ·n H2O(s). If this hydrate is heated to a high enough
temperature, H2O(g) can be driven off, leaving the pale yellow
anhydrous salt FeSO4(s). A 10.140-g sample of the hydrate was
heated to 300 °C. The resulting FeSO4(s) had a mass of 5.5406 g.
Calculate the value of n in FeSO4 ·n H2O(s).
What is the pH of 0.1 M FeSO4 please show all steps
What is the pH of 0.1 M FeSO4 please show all steps
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