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o University of Central learning.com/ibiscms/mod/ibis/view.php?id 2968462 Grad 11/8/2016 os:00 AM CA 17.3/100 10131/2016 07:50 PM Print Calculator Periodic Table uestion 16 of 34 Sapling Learning In a constant-pressure calorimeter, 65.0 mL of 0.300 M Ba(OH 2was added to 65.0 mL of 0.600 MHCI. The reaction caused the temperature of the solution to rise from 22.37 C to 26.46 C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 Jlg C, respectively), what is AH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes. AH kJ mol H,O AePrevious ® Give up s view solution Check Answer Next Ext Hint about us careers partners l privacy policy terms I ow

Explanation / Answer

we know that

moles = molarity x volume (ml) / 1000

so

moles of Ba(OH)2 = 0.3 x 65 / 1000 = 0.0195

moles of HCL = 0.6 x 65 / 1000 = 0.039

now

the reaction is

Ba(OH)2 + 2 HCl --> BaCl2 + 2H20

we can see that

1 mole of Ba(OH)2 reacts with 2 moles of HCL

so 0.0195 moles of Ba(OH)2 will completely react with 0.039 moles of HCl

now

moles of H20 produced = moles of HCl reacted = 0.039

now

final volume of solution = 65 + 65 = 130 ml

now

mass = density x volume

so

mass of solution = 1 x 130 = 130 g

now

heat = mass x specific heat x temp change

heat = 130 x 4.184 x ( 26.46 - 22.37)

heat = 2224.6328 J

now

heat of reaction = heat / moles of H20 produced

heat of reaction = 2224.6328 / 0.039

heat of reaction = 57042

heat of reaction = 57.042

so

the heat of reaction is -57.042 kJ / mol H20 produced

note : the sign is negative because heat is released

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