The species getting oxidized by 1M HBr needs to be identified. Concept introduction: A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction . The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized. An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s. Spontaneity of a reaction is dependent on the free energy sign that is Δ G o . It should be negative for a reaction to be spontaneous. Since, Δ G = − n F E o Here, n = number of electrons involved in reaction and F is faraday constant. If the value of E° for a reaction is positive, then the reaction occurs spontaneous.
The species getting oxidized by 1M HBr needs to be identified. Concept introduction: A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction . The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized. An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s. Spontaneity of a reaction is dependent on the free energy sign that is Δ G o . It should be negative for a reaction to be spontaneous. Since, Δ G = − n F E o Here, n = number of electrons involved in reaction and F is faraday constant. If the value of E° for a reaction is positive, then the reaction occurs spontaneous.
Solution Summary: The author explains that the species getting oxidized by 1M HBr needs to be identified.
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
Chapter 17, Problem 46QAP
Interpretation Introduction
Interpretation:
The species getting oxidized by 1M HBr needs to be identified.
Concept introduction:
A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction. The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized.
An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s.
Spontaneity of a reaction is dependent on the free energy sign that is ΔGo. It should be negative for a reaction to be spontaneous.
Since,
ΔG=−nFEo
Here, n = number of electrons involved in reaction and F is faraday constant.
If the value of E° for a reaction is positive, then the reaction occurs spontaneous.
Identifying the major species in weak acid or weak base equilibria
Your answer is incorrect.
• Row 2: Your answer is incorrect.
• Row 3: Your answer is incorrect.
• Row 6: Your answer is incorrect.
0/5
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
formulas of the species that will act as neither acids nor bases in the 'other' row.
You will find it useful to keep in mind that HF is a weak acid.
acids:
HF
0.1 mol of NaOH is added to
1.0 L of a 0.7M HF
solution.
bases:
0.13 mol of HCl is added to
1.0 L of a solution that is
1.0M in both HF and KF.
Exponent
other:
F
acids: HF
bases: F
other:
K
1
0,0,...
?
000
18
Ar
Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
2NOCI (g) 2NO (g) + Cl2 (g) AGº =41. kJ
Now suppose a reaction vessel is filled with 4.50 atm of nitrosyl chloride (NOCI) and 6.38 atm of chlorine (C12) at 212. °C. Answer the following questions
about this system:
?
rise
Under these conditions, will the pressure of NOCI tend to rise or fall?
x10
fall
Is it possible to reverse this tendency by adding NO?
In other words, if you said the pressure of NOCI will tend to rise, can that
be changed to a tendency to fall by adding NO? Similarly, if you said the
pressure of NOCI will tend to fall, can that be changed to a tendency to
rise by adding NO?
yes
no
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of NO needed to reverse it.
Round your answer to 2 significant digits.
0.035 atm
✓
G
00.
18
Ar
Highlight each glycosidic bond in the molecule below. Then answer the questions in the table under the drawing area.
HO-
HO-
-0
OH
OH
HO
NG
HO-
HO-
OH
OH
OH
OH
NG
OH
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell