Care must be taken when diluting sulfuric acid with water, because the dilution
ID: 900355 • Letter: C
Question
Care must be taken when diluting sulfuric acid with water, because the dilution process is highly exothermic: H2SO4(l) "arrow" H2SO4(aq) + heat a) Find the Ho 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). Suppose you carry out the dilution in a calorimeter. The initial T is 28.8C, and the specific heat capacity of the final solution is 3.50 J/g·K. What is the final T? the first part is -93.52. ( that was marked correct). ..I don't know what the temp is though.. .It said hint: what formula should be used to find the standard enthalpy of a reaction?..it is NOT 377.32 degrees!!!! I NEED FINAL Temperature....
Explanation / Answer
Solution :-
Volume of the final solution = 1 L = 1000 ml
Mass of the final solution = 1000 ml * 1.060 g /ml = 1060 g
Initial temperature = 28.8 C
Final temperature = ?
Delta H dissolution of 1 mol H2SO4 = -93.52 kH * 1000 J / 1 kJ = 93520 J
Specific heat of final solution = 3.50 J /gC
Formula
q= m*s*delta T
93520 J = 1060 g * 3.50 J per g C * delta T
93520 J / 1060 g * 3.50 J per g C = delta T
25.2 C = delta T
Therefore the final temperature = T initial + delta T
= 28.8 C + 25.2 C
= 54.0 C
So the final temperature is 54 C