Diluting sulfuric acid with water is highly exothermic: (a) Use Appendix B to find for diluting 1.00 mol of H2SO4(l) (d = 1.83 g/mL) to 1 L of 1.00 M H2SO4(aq) (d = 1.060 g/mL). (b) Suppose you carry out the dilution in a calorimeter. The initial T is 25.0°C, and the specific heat capacity of the final solution is 3.50 J/g·K. What is the final T? (c) Use the ideas of density and heat capacity to explain why you should add acid to water rather than water to acid.

The final temperature  ° c

Explanation:

(a).

= - 813.9

= - 907.51  

(b).

E = 93520 J

C = 3.5

Initial temperature ° c

Mass (m) = density × volume

m = 1060 × 1

m = 1060 gm

93520 =1060 × 3.5 × ( - 298 )

 ° c

This is the final temperature.

(c).

The density of sulfuric acid is more than the water. so when water is added to acid the mixing process does not takes properly. So we have to add acid in to the water.

Adding water is exothermic process so when we add water to acid than in that case more energy produces and wasted.

i believe the answer is a.

the correct answer is:

a. formation of precipitation