25.00 mL of 0.100 M HCl is mixed with 25.00mL of 1.00 M LiOH in the calorimeter.

Question

25.00 mL of 0.100 M HCl is mixed with 25.00mL of 1.00 M LiOH in the calorimeter. the initial temperature of HCL and LiOH solution is 20.50 deg C, and the equilibrium temperature of the reaction mixture is 38.50 deg C. assume the density and the specific heat of the solution is the same as for water, 1.00g/mL and 4.8184 J/g deg C. a. determine q solution (heat absorbed or released by the reaction mixture)? b. calculate the moles of the limiting reagent in the reaction? c. what is the delta H reaction in kj/mol for the neutralization reaction? d. is the neutralization reaction endothermic or exothermic?

Explanation / Answer

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a)Heat obsorbed by solution=msT

                                          =50*4.8184*18

                                          =4336.56J

b)Moles of limiting reagent=0.1*0.025=0.0025moles of HCL

c)H=4.336/0.0025=1734.4kJ/mole

d)This reaction is exothermic

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