Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0006 molar and everything else is standard (use 298 K for the temperature, R= 8.314 3/mol-K, and F = 96,485 C/mol): (a) 1 Br₂(1) + 2 Li(s) --> 2 Br (aq) + 2 Li¹(aq) (b) 2 Hg²+ (aq) + 2 Hg(1) --> 1 Hg₂+ (aq) + 1 Hg₂²+ (aq) (c) 1 Mg²+ (aq) + 1 Zn(s) --> 1 Mg(s) + 1 Zn²+ (aq) (d) 1 Fe²+ (aq) + 1 Cd(s)--> 1 Fe(s) + 1 Cd²+ (aq) E= E= E= V

Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0006 molar and everything else is standard (use 298 K for the temperature, R= 8.314 3/mol-K, and F = 96,485 C/mol): (a) 1 Br₂(1) + 2 Li(s) --> 2 Br (aq) + 2 Li¹(aq) (b) 2 Hg²+ (aq) + 2 Hg(1) --> 1 Hg₂+ (aq) + 1 Hg₂²+ (aq) (c) 1 Mg²+ (aq) + 1 Zn(s) --> 1 Mg(s) + 1 Zn²+ (aq) (d) 1 Fe²+ (aq) + 1 Cd(s)--> 1 Fe(s) + 1 Cd²+ (aq) E= E= E= V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 112CWP: The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature...

See similar textbooks

Similar questions

9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)
The following reaction occurs in pure water: H2O(l)+H2O(l)H3O+(aq)+OH-(aq) which is often abbreviated as H2O(l)H+(aq)+OH-(aq) For this reaction, G = 79.9 kJ/mol at 25C. Calculate the value of G for this reaction at 25C when [OH] = 0.15 M and [H+] = 0.71 M.
The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).
Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 C to 17.1 C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
The equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.