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Question

50.0mL of 0.10M HCl is mixed with 50.0mL of 0.10M NaOH. The solution temperature rises by 3.0oC. Calculate the enthalpy of neutralisation per mol of HCl.

A
2.5×102kJ
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B
1.3×102kJ
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C
8.4×101kJ
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D
6.3×101kJ
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Solution

The correct option is C 2.5×102kJ
No. of moles of HCl=5 milimoles
No. of moles of NaOH=5 millimoles
Mass of solution mixed =50 gm+50 gm=100 gm
ΔH=cmΔT(c=4.18 kJKg1)
ΔH=4.18×0.1×3
ΔH=1.254 kJ (For 5 milimoles of water formed)
For 1 mole water =1.2545×103=2.5×102 kJ

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