The chemical reaction between the reactants:
3 AgNO₃ (aq) + FeCl₃ (aq) → 3 AgCl (s) + Fe(NO₃)₃ (aq)
Explanation:
We have the following chemical reaction:
3 AgNO₃ (aq) + FeCl₃ (aq) → 3 AgCl (s) + Fe(NO₃)₃ (aq)
Complete ionic equation:
3 Ag⁺ (aq) + 3 NO₃⁻ (aq) + Fe³⁺ (aq) + 3 Cl⁻ (aq) → 3 AgCl (s) + Fe³⁺ (aq) + 3 NO₃⁻ (aq)
We remove the spectator ions and we get the net ionic equation:
Ag⁺ (aq) + Cl⁻ (aq) → AgCl (s)
where:
(aq) - aqueous
(s) - solid
Learn more about:
net ionic equation
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Answer:
relative humidity
Explanation:
Relative humidity can be measured with a hygrometer
HCl:
<span>
m=48,2g
M=36,5g/mol
n = m/M = 48,2g / 36,5g/mol = 1,32mol
1mol : 4mol
MnO</span>₂ + 4HCl ⇒ MnCl₂ + Cl₂ + 2H₂O
0,86mol : 1,32mol
limiting reagent
0,33 will react
HCl is limiting reagent.
Answer:
Multiple organisms may be affected by the loss of a plant species.
Explanation:
Organisms that feed directly off the lost plant will be affected, and because of that, organisms that feed off those organisms will be affected. This could also affect other organisms like parasites. Other plant species may be affected from the loss of a competitive species. This could affect organisms that feed off that plant, and the organisms that feed off those organisms.
E
θ
Cell
=
+
2.115
l
V
Cathode
Mg
2
+
/
Mg
Anode
Ni
2
+
/
Ni
Explanation:
Look up the reduction potential for each cell in question on a table of standard electrode potential like this one from Chemistry LibreTexts. [1]
Mg
2
+
(
a
q
)
+
2
l
e
−
→
Mg
(
s
)
−
E
θ
=
−
2.372
l
V
Ni
2
+
(
a
q
)
+
2
l
e
−
→
Ni
(
s
)
−
E
θ
=
−
0.257
l
V
The standard reduction potential
E
θ
resembles the electrode's strength as an oxidizing agent and equivalently its tendency to get reduced. The reduction potential of a Platinum-Hydrogen Electrode under standard conditions (
298
l
K
,
1.00
l
kPa
) is defined as
0
l
V
for reference. [2]
A cell with a high reduction potential indicates a strong oxidizing agent- vice versa for a cell with low reduction potentials.
Two half cells connected with an external circuit and a salt bridge make a galvanic cell; the half-cell with the higher
E
θ
and thus higher likelihood to be reduced will experience reduction and act as the cathode, whereas the half-cell with a lower
E
θ
will experience oxidation and act the anode.
E
θ
(
Ni
2
+
/
Ni
)
>
E
θ
(
Mg
2
+
/
Mg
)
Therefore in this galvanic cell, the
Ni
2
+
/
Ni
half-cell will experience reduction and act as the cathode and the
Mg
2
+
/
Mg
the anode.
The standard cell potential of a galvanic cell equals the standard reduction potential of the cathode minus that of the anode. That is:
E
θ
cell
=
E
θ
(
Cathode
)
−
E
θ
(
Anode
)
E
θ
cell
=
−
0.257
−
(
−
2.372
)
E
θ
cell
=
+
2.115
Indicating that connecting the two cells will generate a potential difference of
+
2.115
l
V
across the two cells.
