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1. A chemical reaction was conducted at several different temperatures (measured in K) and the equilibrium constant was measured at each one. Plotting the data on a graph with ln K on the y-axis and 1/T on the x-axis gives a linear plot with slope = -4594.6 and y-intercept = 13.6. What is ΔrH° (in kJ mol-1 ) and ΔrS° (in J mol-1 K -1 )?
2. Consider the galvanic cell:
Al (s) | Al3+ (aq, 0.018 mol L-1 ) || Fe2+ (aq, 0.85 mol L-1 ) | Fe (s)
a) Write out the overall reaction taking place in this cell.
b) Calculate E°cell for this cell at 298 K to two decimal places.
c) Calculate Ecell for this cell at 298 K to two decimal places.
d) If this cell is allowed to operate, will Ecell increase, decrease or remain constant over time? Briefly explain.
3. For the following reaction at 500 K:
Calculate the temperature of the system once equilibrium has been reached. Assume that Cp,m for Au and H2O is constant at its value for 298K throughout the temperature range of interest.
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