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88 solutions

The Nernst Equation

Q. Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cr^3+(aq) +Co(s) → 2Cr^2+(aq) + Co^2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. ΔG° for this reaction would be ____ than zero.

Solved • Nov 16, 2019

The Nernst Equation

Q. What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the H2 pressure is 7.30x10^-3 atm, the H^+ concentrations is 1.34 M, and the Sn^+ concentration is 3.95x10^-4M? 2H^+(aq) + Sn(s) → H2(g) + Sn^2+(aq) The cell reaction as written above is spontaneous for the concentrations given:

Solved • Nov 16, 2019

The Nernst Equation

Q. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Ni2(aq) + Fe(s) → Ni(s) + Fe^2+(aq) K for this reaction would be ____ than one.

Solved • Nov 16, 2019

The Nernst Equation

Q. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.43 atm, the F^- concentrations is 9.37x10^-3M, and the Cr^3+ concentrations is 2.65x10^-4M? 3F2(g) + 2Cr(s) → 6.00F^-(aq) + Cr^3+(aq) Answer: ____ V The cell reaction as written above is spontaneous for the concentrations given: ____

Solved • Nov 14, 2019

The Nernst Equation

Q. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H2 pressure is 4.24x10^-3 atm, the H^+ concentrations is 1.04M, and the Mg^2+ concentrations is 1.2x10^-4M? 2H^+(aq) + Mg(s) → H2(g) + Mg^2+(aq) Answer: ____ V The cell reaction as written above is spontaneous for the concentrations given: ____

Solved • Nov 14, 2019

The Nernst Equation

Q. Consider then galvanic cell based on the following half-reactions: Mn^2+ + 2e^- → Mn E° = -1.18 V Fe^2+ + 2e^- → Fe E° = -0.44 V c. Calculate Ecell at 25 °C when [Mn^2+] = 0.10 M and [Fe^2+] = 4.0 x 10^-6 M.

Solved • Nov 14, 2019

The Nernst Equation

Q. Consider the cell described below: Zn|Zn^2+ (1.00 M)||Cu^2+(1.00 M)| Cu Calculate the cell potential after the reaction has operated long enough for the [Zn^2+] to have changed by 0.44 mol/L. (Assume T = 25 °C.) (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 Mindtap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.)

Solved • Nov 14, 2019