Part E
Write a balanced chemical equation depicting the formation of
one mole of POCl3(l) from its elements in their standard
states.
Express your answer as a chemical equation. Identify all of the
phases in your answer.
14P4(s)+12O2(g)+112Cl3(g)→POCl3(l)
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Part F
For POCl3(l), find the value of ΔH∘f.
(Use Appendix C in the textbook).
Express...
For each reaction write a balanced chemical equation and then
below the chemical formula of each reactant and product write a
brief description of the substance (color and physical state).
Also, indicate whether the reaction is exothermic, endothermic, or
cannot tell.
1. Combination Reaction
Equation:
Exothermic
Endothermic
Cannot tell
Evidence of Chemical Change:
2. Reversible Decomposition--Combination
Reactions
Dehydration of Blue Vitrol (Copper(II) Sulfate
Pentahydrate)
Equation:
CuSO4·5H2O ® CuSO4 +
5H2O
Exothermic
Endothermic
Cannot tell
Evidence of Chemical Change:
Rehydration...
Use the following half-reactions to write three spontaneous
reactions, and calculate E cell for each reaction:
a. Au+ (aq) + e- ----> Au (s) E= 1.69
V
b. N2O (g) + 2H+ (aq) + 2 e-
----> N2 (g) + H2O (l) E= 1.77 V
c. Cr3+ (aq) + 3e- ---> Cr (s) E= -0.74
V
Write a balanced molecular equation for the reaction of each of
the following metals with dilute hydrochloric acid. If no reaction
occurs, put NR. (a) Ni (b) Fe (c) Ag (d) Au
2. Write a balanced chemical equation for the reaction of one
anion in each of the categories in question 1.
A. a precipitation reaction
B. a redox reaction
C. an acid-base reaction
D. a gas-forming reaction
The Equations Given:
Ca+2(aq) + SO4 -2(aq) ↔ CaSO4(s) Equation 1
Ca+2(aq) + CO3 -2(aq) ↔ CaCO3(s) Equation 2
CaCO3(s) + 2H+ (aq) → Ca+2(aq) + CO2(g) + H2O(l) Equation 3
CaSO4(s) + H+ (aq) → No Reaction (precipitate remains) Equation
4
2NO2 -...
Consider each of the following ionic compounds and write (a) a
balanced equation for Ksp for their dissolution and (b) given their
Ksp values calculate the molar solubility of each.
BaCrO4 (Ksp = 1.17 x 10-10)
Ca3(PO4)2 (Ksp = 2.07 x 10-33)
Ag2S (Ksp = 6.00 x 10-51)
Write the balanced equation for each of the chemical
reactions:
a) Solid sodium is added to water and reacts to form a solution
of sodium hydroxide.
b) Solid cobalt (III) oxide reacts with carbon to produce cobalt
metal and carbon dioxide.
c) The fermentation of sugar, C12H22O11, in which aqueous sugar
reacts with water to form aqueous ethanol, C2h5OH, and carbon
dioxide gas.
d) Solid metallic aluminum reacts with aqueous hydrochloric acid
to produce aqueous aluminum chloride and hydrogen gas.
Given the balanced equation: 3Ni(s) + 2Au3+(aq) :⟶2Au(s) +
3Ni2+(aq), E^o_{cell}\:E c e l l o= 1.76 V, what is the cell
potential for this reaction when [Au3+] = 0.95 M and [Ni2+] = 0.016
M at 298 K? Group of answer choices
1.78 V
1.71 V
1.81 V
1.92 V