Reaction 1: Cu(s) + AgNO3 (aq) = CuNO3 (aq) + Ag (s)
Reaction 2: Cu (s) +AgNO3 (aq) = Cu(NO3)2 (aq) + Ag (s)
Part 1: Write the balanced net ionic equations for both of the
above reactions.
Assume that excess silver nitrate is available when answering
the remaining questions.
Part 2: Calculate the theoretical grams of silver metal that
could form from 2.568g of copper wire based upon reaction 1. (Be
sure the reaction is properly balanced.)
Part 3:...
Calculate ΔG° for the following reaction as written
Ni2+ (aq) + Sn (s) → Ni (s) + Sn2+
(aq)
given the following reduction half-reactions and standard
reduction potentials.
Sn2+ (aq) + 2 e- → Sn (s)
E° = -0.15V
Ni2+ (aq) + 2 e- → Ni (s)
E° = -0.25V
For the following reaction: Ni2+(aq) + Co(s) ⇌ Ni(s) +
Co2+(aq)
a) Calculate E0 (E^0)
b) Calculate G0 (delta G^0)
c)Calculate K
d) If you start with 10.0 g of Ni and 10.0 g of Co in 100.0 mL
solution (containing 1.0 M solution of CoCl2 and 0.0000100 M
solution of NiCl2 ) which way the reaction will move toward in
order to reach equilibrium?
e) Calculate the G (delta G) for the reaction in part d.
f)Calculate the equilibrium...
Part A
Calculate the equilibrium constant at 25 ∘C for the
reaction
Ni(s)+2Ag+(aq)→Ni2+(aq)+2Ag(s),
if
Ni2+(aq)+2e−→Ni(s), E∘
= -0.26 V,
Al+(aq)+e−→Al(s), E∘ =
0.80 V
Express your answer using one significant figure.
Part B
Calculate the equilibrium constant at 25 ∘C for the
reaction
Hg2+2(aq)→Hg(l)+Hg2+(aq)
See Appendix D for standard reduction potentials.
Express your answer using one significant figure.
Consider the balanced chemical reaction Cu(s) + 2AgNO3(aq) a
2Ag(s) + Cu(NO3)2(aq)
a) Write the Complete Ionic Equation:
b) Write the Net Ionic Equation:
c) Assign oxidation numbers to all of atoms/ions in the
reaction:
Cu _____ Ag _____ NO3_____ a Ag _____ Cu _____ NO3 _____
d) Which atom/ion is being oxidized in this reaction?
e) Which atom/ion is being reduced in this reaction?
Homework Text bOOK
Here is the reaction
Cu (s) + 4 HNO3 (aq) >>> Cu(NO3)2 (aq) + 2
NO2 (g) + 2 H2O (l) You are given 1.00 g of copper, how much
concentrated nitric acid (in mL) do you need for this reaction?
Concentrated nitric acid is 15.0 M HNO3. Which is the
correct answer:
4.19
6.29
1.05
8.38
You are given 1.00 g of copper and 5.00 mL of concentrated
nitric acid, how much concentrated nitric acid (in mole)...
Given the following reaction, Cu2+(aq) + Zn(s) → Cu(s) +
Zn2+(aq) E° = 1.10 V.
Use the Nernst equation to calculate the cell potential for the
cell described with standard line notation below.
Zn|Zn2+(0.5082 M)||Cu2+(0.2699 M)|Cu
Units are not required. Report answer to three decimal
places.
Please explain all of your steps! Thanks!
Answer the following for the reaction:
NiCl2(aq)+2NaOH(aq)→Ni(OH)2(s)+2NaCl(aq)
How many grams of Ni(OH)2 are produced from the
reaction of 41.0 mLof a 1.95 M NaOH solution and excess
NiCl2?
Express your answer with the appropriate units.
Consider the following reaction:
2 Al + 3 CuCl2 → 3 Cu + 2 AlCl3
The reaction begins with 83.16 g of Al and 49.19 g of copper II
chloride.
How much of the excess reactant is left behind
(unused)? g
How many grams of Cu is produced: g
How many grams of AlCl3 is produced: g
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 ?