The reaction happening will be Ba(OH)2(aq) + 2HCl(aq) ------- BaCl2(s) + 2H2O(l)

Question

The reaction happening will be

Ba(OH)2(aq) + 2HCl(aq) ------- BaCl2(s) + 2H2O(l)

Number of moles of Ba(OH)2 = Volume of solution in L * Molarity = 55/1000 * 0.330 = 0.01815 moles

Number of moles of HCl = Volume of solution in L * Molarity = 55/1000 * 0.660 = 0.0363 moles

Since Ba(OH)2 1 mole requires 2 moles of HCl and the number of HCl is exactly 2 times the Ba(OH)2 moles

Hence both the reactants will be utilized to 100%

Number of moles of H2O formed = Number of moles of HCl = 0.0363 moles

mass of H2O formed = 0.0363 mol * 18.015 gm/mol = 0.6539 grams

mass of solution = 55 mL + 55 mL = 110 mL

Since density is assumed to be as water = 1 gm/mL

Mass of solution = 110 gm

Specific heat of water = 4.18 J/gC

Change in Temperature = Final Temp - Initial Temp = 26.93 - 22.43 = 4.5

q = 110g * 4.18 J/gC * 4.5C = 2069.1 J

Hence Delta H(rxn) = -2069.1 J per 0.0363 moles

Delta H(rxn) per mole of water = -2069.1/0.0363 = -57000 J = -57 kJ

Explanation / Answer

In a constant-pressure calorimeter, 55.0 mL of 0.330 M Ba(OH2 was added to 55.0 mL of 0.660 M HC The reaction caused the temperature of the solution to rise from 22.43 to 26.93 . If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ) Number 57.1 kJ

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