1) Balance the following reaction under acidic conditions and calculate the cell potential in (V) at...
1)
Balance the following reaction under acidic conditions and calculate the cell potential in (V) at 298 K generated by the cell. Report your answer to the hundredths place.
Cr2O72-(aq) + I-(aq) → Cr3+(aq) + I2(s)
[Cr2O72-] = 2.0 M, [H+] = 1.0 M, [I-] = 1.0 M, [Cr3+] = 1.0 × 10-5 M
2) What is the value of n for the following reaction? Enter the whole number.
3Ni+(aq) + Cr(OH)3(s) + 5OH-(aq) → 3Ni(s) + CrO42-(aq) + 4H2O(l)
Homework Answers
![OV 0.059 Ecev = 0.80V - D50 hoy (50 x 10) 2 0.80 v = 0.00385 lag., (5 % 10-19 2 0.80V - 0.00985 { 19.5 -11] 01/1Y 2 0.80 V -](http://img.homeworklib.com/questions/7d6caaa0-c5df-11eb-86ce-872802fe4182.png?x-oss-process=image/resize,w_560)
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1)
Balance the following reaction under acidic conditions and
calculate the cell potential in (V) at...
Using the Nernst equation, calculate the cell potential for the following reaction (T=298 K): Cr2O72- (aq)...
Using the Nernst equation, calculate the cell potential for the following reaction (T=298 K): Cr2O72- (aq) + 14 H+ (aq) 6 I- (aq) → 2 Cr3+ (aq) + 3 I2 (s) + 7 H2O (l) given that Cr2O72- = 1.7 M H+ = 1 M I- = 1 M Cr3+ = 0.002 M
Predict cell potential under nonstandard conditions. What is the calculated value of the cell potential at...
Predict cell potential under nonstandard conditions. What is the calculated value of the cell potential at 298K for an electrochemical cell with the reaction shown below, when the [Hg2+ ]= 1.13 M and the [ Cr3+ ] = 9.02x10-4 M? 3 Hg2+ (aq) + 2 Cr (5) —— 3 Hg (1) + 2 Cr3+ (aq) Cell Potential: V
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) MnO4-(aq)...
Balance the following equations. (Use the lowest possible
whole-number coefficients. These may be zero.)
(a) MnO4-(aq) + Cl-(aq) Mn2+(aq) + Cl2(aq)
MnO4- + Cl-
+ H+ + H2O Mn2+
+ Cl2 + H+
+ H2O
(b) Cr2O72-(aq) +
NO2-(aq) Cr3+(aq) +
NO3-(aq)
Cr2O72-
+ NO2- + H+
+ H2O Cr3+
+ NO3- + H+
+ H2O
(c) Tl2O3(s) + NH2OH(aq) TlOH(s) + N2(g)
Tl2O3 + NH2OH
+ OH- + H2O TlOH(s) + N2
+ OH- + H2O
(d) CrO42-(aq) +
C2O42-(aq) Cr(OH)3(s) +
CO2(g)
CrO42-
+ C2O42-
+ OH- + H2O Cr(OH)3
+ CO2 + OH-
+ H2O
1.A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s)...
1.A voltaic cell is constructed that uses the following reaction
and operates at 298 K.
Zn(s) + Ni2+(aq)
Zn2+(aq) + Ni(s)
2.A voltaic cell utilizes the following reaction and operates at
298 K.
3 Ce4+(aq) + Cr(s)
3 Ce3+(aq) + Cr3+(aq)
We were unable to transcribe this imageA voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) → Zn2+ (aq) + Ni(s) (a) What is the emf of this cell under standard...
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s)...
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions? _____V (b) What is the emf of this cell when [Ce4+] = 1.2 M, [Ce3+] = 0.010 M, and [Cr3+] = 0.012 M? ____V (c) What is the emf of the cell when [Ce4+] = 0.53 M, [Ce3+] = 0.89 M, and [Cr3+] = 1.0 M? ____V
For each of the following reactions, balance the chemical equation, calculate the emf, and calculate G°...
For each of the following reactions, balance the chemical
equation, calculate the emf, and calculate G° at 298 K. (Use the smallest possible
coefficients for H2O(l),
H+(aq), and HO-(aq). These
may be zero.)
(a) In acidic solution copper(I) ion is oxidized to copper(II)
ion by nitrate ion.
Cu+(aq)
+ NO3-(aq)
+ H+(aq) Cu2+(aq) NO(g)
+ H2O(l)
emf
V
G°
kJ
(b) Aqueous iodide ion is oxidized to I2(s) by
Hg22+(aq).
I-(aq)
+ Hg22+(aq)
+ H+ I2(s) Hg(l)
+ H2O(l)
emf
V
G°
kJ
(c) In basic solution Cr(OH)3(s) is...
3. + -10.1 points 0/4 Submissions Used A voltaic cell utilizes the following reaction and operates...
3. + -10.1 points 0/4 Submissions Used A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+ (aq) + Cr(s) + 3 Ce3+ (aq) + Cr3+ (aq) (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when [Ce4+] = 2.0 M, (Ce3+] = 0.010 M, and [Cr3+] = 0.010 M? (c) What is the emf of the cell when [Ce4+] = 0.52 M, [Ce3+] = 0.84...
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an el...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
3. Calculate the cell potential for the voltaic cell based on the following half reactions at...
3. Calculate the cell potential for the voltaic cell based on the following half reactions at T = 25°C: Cr3+(aq) + 3e Cr(s) E° = -0.74 V TiO2(aq) + 2H(aq) + 1e → Ti+(aq) + H2O(1) E° = + 0.10 V Where, [Cr3+] = 1.0 x 104 M, [TiO2+] = 1.0 x 10-1M, [H+] = 1.0 M, [Ti$+] = 5.0 x 10-2 M.
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2...
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures. H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq) The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. Pt(s) l Cr3+(aq),...
Predict cell potential under nonstandard conditions. What is the calculated value of the cell potential at 298K for an electrochemical cell with the reaction shown below, when the [Hg2+ ]= 1.13 M and the [ Cr3+ ] = 9.02x10-4 M? 3 Hg2+ (aq) + 2 Cr (5) —— 3 Hg (1) + 2 Cr3+ (aq) Cell Potential: V
Balance the following equations. (Use the lowest possible
whole-number coefficients. These may be zero.)
(a) MnO4-(aq) + Cl-(aq) Mn2+(aq) + Cl2(aq)
MnO4- + Cl-
+ H+ + H2O Mn2+
+ Cl2 + H+
+ H2O
(b) Cr2O72-(aq) +
NO2-(aq) Cr3+(aq) +
NO3-(aq)
Cr2O72-
+ NO2- + H+
+ H2O Cr3+
+ NO3- + H+
+ H2O
(c) Tl2O3(s) + NH2OH(aq) TlOH(s) + N2(g)
Tl2O3 + NH2OH
+ OH- + H2O TlOH(s) + N2
+ OH- + H2O
(d) CrO42-(aq) +
C2O42-(aq) Cr(OH)3(s) +
CO2(g)
CrO42-
+ C2O42-
+ OH- + H2O Cr(OH)3
+ CO2 + OH-
+ H2O
1.A voltaic cell is constructed that uses the following reaction
and operates at 298 K.
Zn(s) + Ni2+(aq)
Zn2+(aq) + Ni(s)
2.A voltaic cell utilizes the following reaction and operates at
298 K.
3 Ce4+(aq) + Cr(s)
3 Ce3+(aq) + Cr3+(aq)
We were unable to transcribe this imageA voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) → Zn2+ (aq) + Ni(s) (a) What is the emf of this cell under standard...
For each of the following reactions, balance the chemical
equation, calculate the emf, and calculate G° at 298 K. (Use the smallest possible
coefficients for H2O(l),
H+(aq), and HO-(aq). These
may be zero.)
(a) In acidic solution copper(I) ion is oxidized to copper(II)
ion by nitrate ion.
Cu+(aq)
+ NO3-(aq)
+ H+(aq) Cu2+(aq) NO(g)
+ H2O(l)
emf
V
G°
kJ
(b) Aqueous iodide ion is oxidized to I2(s) by
Hg22+(aq).
I-(aq)
+ Hg22+(aq)
+ H+ I2(s) Hg(l)
+ H2O(l)
emf
V
G°
kJ
(c) In basic solution Cr(OH)3(s) is...
3. + -10.1 points 0/4 Submissions Used A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+ (aq) + Cr(s) + 3 Ce3+ (aq) + Cr3+ (aq) (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when [Ce4+] = 2.0 M, (Ce3+] = 0.010 M, and [Cr3+] = 0.010 M? (c) What is the emf of the cell when [Ce4+] = 0.52 M, [Ce3+] = 0.84...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
3. Calculate the cell potential for the voltaic cell based on the following half reactions at T = 25°C: Cr3+(aq) + 3e Cr(s) E° = -0.74 V TiO2(aq) + 2H(aq) + 1e → Ti+(aq) + H2O(1) E° = + 0.10 V Where, [Cr3+] = 1.0 x 104 M, [TiO2+] = 1.0 x 10-1M, [H+] = 1.0 M, [Ti$+] = 5.0 x 10-2 M.
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