An electrolysis cell is operated for 3000 s using a current of
1.50 A. From which...
An electrolysis cell is operated for 3000 s using a current of
1.50 A. From which 1.0 M solution will the greatest mass of metal
be deposited? Answer is A please explain
Molten ZnBr2 is electrolyzed by passing a current of 15.0 A through
an electrolysis cell for a certain length of time. In this process,
45.75g Br2 are deposited_________( anode or cathode). How long does
this process require? What is the chemical reaction taking place at
the other electrode? What mass of the second product is released at
the other electrode?
A current of 6.15×104
A is passed through an electrolysis cell
containing molten MgCl2 for
6.50 days.
(a) How many grams of magnesium
are produced?
_____g
(b) How many liters of chlorine
are collected, if the gas is at a temperature of
273 K and a pressure of 1.00
atm?
_____L
For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155
M)||Ag (aq, 1.50 M)|Ag(s)
write the net cell equation. Phases are optional. Do not include
the concentrations.
Calculate the following values at 25.0 °C using standard
potentials as needed.
E cell #1:
E cell #2:
G rxn #1:
Grxn#2:
there will be 4 answers total!
Copper can be electroplated at the cathode of an electrolysis
cell by the half-reaction.
Cu2+(aq)+2e−→Cu(s)Cu2+(aq)+2e−→Cu(s)
Part A
How much time would it take for 338 mgmg of copper to be plated
at a current of 7.1 AA ?
A voltaic cell is constructed from
an Ni2+(aq)−Ni(s) half-cell and
an Ag+(aq)−Ag(s) half-cell.
The initial concentration of Ni2+(aq) in the
Ni2+−Ni half-cell is [Ni2+]= 1.80×10−2 M . The initial
cell voltage is +1.12 V .
Part A
By using data in Table 20.1 in the textbook, calculate the
standard emf of this voltaic cell.
E∘ =
V
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Part B
Will the concentration of Ni2+(aq) increase or
decrease as the cell operates?
Will the concentration of increase or...
The standard emf for the cell using the overall cell reaction
below is +2.20 V:
2Al(s) + 3I2(s) →→ 2AI3+(aq) +
6I-(aq)
The emf generated by the cell when [AI3+] = 3.5 ×
10-3 M and [I-] = 0.30 M is ________ V.
Devise a cell for which the full cell reaction is:
Ag+(aq) + Br−(aq) → AgBr
(s)
a. What is the cell emf at 25°C?
b. Calculate DG˚rxn from both E° and standard Gibbs energies of
formation.
c. Calculate the equilibrium constant.
d. Calculate the solubility, S, of AgBr.
A 1000 kg car traveling 60° south from east at 30 m/s collides with
a 3000 kg truck traveling north at
20 m/s. The cars stick together after the collision.
a) Is the momentum of the tr uck conserved before and after the
collision? Why?
b) Is the momentum of the car and tr uck together conserved before
and after the collision?
Why?
c) Draw the velocity vector for the car before collision and write
down the x and y...
Consider the Daniell cell, for which the overall cell reaction
is Zn(s)+Cu2+(aq)⇌Zn2+(aq)+Cu(s) The concentrations of CuSO4 and
ZnSO4 are 2.20×10−3 m and 1.10×10−3 m ,
respectively.
A)
Calculate E setting the activities of the ionic species equal to
their molalities.
Express your answer to four significant figures and include the
appropriate units.
B)
Calculate γ±,ZnSO4 for the half-cell solutions using the
Debye-Huckel limiting law.
Express your answer using three significant figures.
C)
Calculate γ±,CuSO4 for the half-cell solutions using the...
Which of the following cell types are formed from a myloid
precursor?
mast cell
B cell
dendritic cell
natural killer cell
macrophage
neutrophil
plasma cell
T cell
Which compliment pathway results in the production of MAC?
Alternative Pathway
Classic Pathway
Manose-binding Lectin Pathway