Suppose that the calorimeter shown here was used to determinethe energy change f

Question

Suppose that the calorimeter shown here was used to determinethe energy change for an acid-base reaction.

An acid/base reaction solution was made by combining 150 mL of 0.5 M HCl of 50 mL of 1.00 M NaOH, to make 200.0g of solution

Other data for the system include:


Initial temperature of solution
36.3C

Specific heat capacity of solution
4.184 J/gC

Enthalpy change for neutralization
-56 kJ/mol
Assume the volumes of acid and base are additive.

Calculate the final temperature of the reaction mixture (assumingno heat loss to the surroundings).

Explanation / Answer

another possible answer: as enthalpy of neutralization is is -56KJ/mol the reaction is NaOH + HCl ---> NaCl + H2O so 56KJ energy is released when 1 equivalent of base and acid react. we have 150ml of 0.5M HCl and 50 ml of 1M NaOH based on stoichiometry only 0.05 mol of NaOH and 0.075 moles of HCl are available. so as NaOH is limiting reactant, only 0.05 moles of NaCl will be formed and heat liberated by reaction will be 0.05(56000) = 2800J now this energy is absorbed by system as there is no heat loss. assume negligible change in mass, const sp.heat and let final temp be T so heat absorbed = m*c*dT so, 2800 = 200*4.184*(T-36.3) solving T = 39.65 degC

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