moles of acid HCl = 50 x 0.660 / 1000 = 0.033 moles of Ba(OH)2 = 50 x 0.330 / 10
ID: 699877 • Letter: M
Question
moles of acid HCl = 50 x 0.660 / 1000 = 0.033
moles of Ba(OH)2 = 50 x 0.330 / 1000 = 0.0165
2 HCl + Ba(OH)2 ------------------------> BaCl2 + 2H2O
2 1
0.033 0.0165 0.033
here both are consumed
moles of water fomred = 0.033
total volume = 50 + 50 = 100 mL
mass of solution = volume x density
= 100 x 1
=100g
dT = 26.35 -21.85= 4.5 oC
Q = 100 x 4.184 x 4.5
Q = 1883 J
H =molar enthalpy of neutralization = - Q / n
= -1.883 / 0.033
= - 57.0 kJ / mol
Explanation / Answer
In a constant-pressure calorimeter, 50.0 mL of 0.330 M Ba(OH)2 was added to 50.0 mL of 0.660 M HCl. The reaction caused the temperature of the solution to rise from 21.85 °C to 26.35 °C. what is H for this reaction (KJ released per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes and that the density and heat capacity are equal to that of water.
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