please help me.. Two solutions namely, 500mL of 0.50M HCl and 500mL of 0.50MNaOH

Question

please help me.. Two solutions namely, 500mL of 0.50M HCl and 500mL of 0.50MNaOH at the same temperature of 22.0 0C are mixed in aconstant pressure calorimeter. The heat capacity of the calorimeterwas 350 J/0C. Given that the specific heat of thesolution is 4.184 J/g 0C the density of the solution is1.00g/mL, and that the heat of neutralization for the processH+ (aq) + OH- (aq) -> H20 (l)is -56.2 kJ, what is the final temperature of the mixedsolution? please help me.. Two solutions namely, 500mL of 0.50M HCl and 500mL of 0.50MNaOH at the same temperature of 22.0 0C are mixed in aconstant pressure calorimeter. The heat capacity of the calorimeterwas 350 J/0C. Given that the specific heat of thesolution is 4.184 J/g 0C the density of the solution is1.00g/mL, and that the heat of neutralization for the processH+ (aq) + OH- (aq) -> H20 (l)is -56.2 kJ, what is the final temperature of the mixedsolution?

Explanation / Answer

      Let the final temperaturebe T2     total volume of the solution =500+500 = 1000 mL     density = 1.00 g /mL    mass of solution = 1000 g          q =msT             qsolution = 1000g*4.184J /oC * (T2-22oC)                    qcalorimetre = heat capacity * T                             =350 J /oC * (T2-22oC)                                        given q rxn = -56.2 kJ = -56.2*103 J                  q rxn = - (q solution +  q calorimetre )           -56.2 *103 J = - (1000g*4.184J /oC * (T2-22oC) + 350 J /oC * (T2-22oC) )                          T2-22oC = - 12.395 oC               T2 = 9.604 oC              

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