Using the Data See assigned by your instructor, determine the heat of solution f

Question

Using the Data See assigned by your instructor, determine the heat of solution for the indicated compound. In each case the amount of solute indicated is dissolved in 50.00 mL of water. Summarize the data in the table provided. Calculate the heat gained or lost by the solution, q_soln. SHOW ALL OF YOLK WORK! (Assume that the specific heat of solution = specific heat of water = 4.184 J/8 times degree C) Calculate the heat of dissolution, Delta H_rxn, in kJ/mol of solute. SHOW ALL OF YOUR WORK! Is the process endothermic or exothermic?

Explanation / Answer

A)

Qgained by solution

Q = m*C*(Tf-Ti)

V = 50 mL = 50 g of water

total mass = 50+4.5 = 54.5 g

assumC = 4.184 J/gC

so

Q = (54.5)(4.184)(38.84-21) = 4068.01 J

b)

for heat of dissolution...

first find moles of H2SO4:

MW of H2SO4 = 98g/mol

mol = mass/MW = 4.5/98 = 0.0459183 mol of H2SO4

so..

HRxn = -Q/n = -(4068.01 J ) / 0.0459183 mol of H2SO4 = -88592.34 J/mol= -88.59 kJ/mol

this must be exothermic process, sicne heat is being released, and HRxn is negative

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