In: Chemistry
Assume you mix (1.25x10^2) mL of 0.400 M HCl with the same volume of 0.400 M NaOH in a coffee-cup calorimeter (as will be done in the lab). The temperature of the solution before the mixing was 25.10 deg. C; after mixing and allowing the reaction to occur, the temperature is 27.78 Deg. C. What is the enthalpy of neutralization of the acid. Assume the densities of all the solutions are 1.00 g/mL and their specific heat capacities are 4.18 J/(g*K)
no of moles of HCl = molarity * volume in L
= 0.4*0.125 = 0.05 moles
no of moles of NaOH = molarity * volume in L
= 0.4*0.125 = 0.05 moles
Total volume of solution = 125 + 125 = 250ml
mass of solution = volume of solution * density
= 250*1 = 250g
q = mcT
= 250*4.18*(27.78-25.1)
= 2800.6J
H = -2800.6J/0.05moles = -56012J/mole = -56.012KJ/mole >>>>>answer