One g-mole of pure liquid sulfuric acid at temperature T0 (°C) is mixed with r g-moles of liquid water, also at temperature T0 (°C), in an adiabatic container. The final solution temperature is Ts (°C). The mass heat capacities of the pure acid, pure water, and the product solution [J/(g?°C)I are Cpa, Cpw, and Cps respectively all of which may be taken to be constant (independent of temperature).

(a) Without doing any calculations, sketch the plot of Ts versus r you would expect to obtain for r varying between 0 and ?.

(b) Use an energy balance to derive an expression for Ts in terms of the initial acid and water temperatures, the heat capacities the water/acid mole ratio (r), and the heat of mixing, ?Hm (r, 25 °C) (kJ/mol H2SO4).

(c) A series of 1.00 mol samples of pure liquid sulfuric acid are added to 11 insulated flasks containing varying amounts of water. The quantities of water in the flasks and the mass heat capacities of the product solutions are tabulated below: The heat capacities of pure sulfuric acid and pure water may be determined from the molar heat capacities in Table B.2 evaluated at 25°C. All heat capacities should be taken to be independent of temperature. Unfortunately, the laboratory air conditioner has been out of order for three weeks (Physical Plant promises they will get to it any day now) and the temperature on the July afternoon of the experiment (which also equals the initial acid and water temperatures) is an uncomfortable 40°C. Write a spreadsheet to generate a table and then a plot of T, the final temperature in each flask, versus r, the water/acid mole ratio of the solution in the flask. (Suggestion: Make the r axis logarithmic.) Assume that mixing is adiabatic.

(d) The actual experimental plot of Ts versus r would lie below the one determined in part (c). Why?

Transcribed Image Text:

r (mol H₂O) 0.5 C, [J/(g°C)] | 158 1.0 1.5 2.0 3.0 4.0 5.0 10.0 25.0 50.0 100.0 1.85 1.89 1.94 2.10 2.27 2.43 3.03 3.56 3.84 4.00