When 50.0 mL of 1.00 M HCl was mixed with 50.0 mL of 1.00 M NaOH in a calorimete

Question

When 50.0 mL of 1.00 M HCl was mixed with 50.0 mL of 1.00 M NaOH in a calorimeter, the temperature rose from 25.0 ºC to 31.5ºC. Calculate the heat change for the reaction, assuming that the total volume of the solution is 100.0 mL of density 1.0 g/mL, and specific heat

1.00 cal/ (g. ºC).

a). write a balanced equation for the reaction

b). how many moles of HCl (aq) and NaOH have reacted?

c). is the reaction exothermic or endothermic?

d). how many calories are evolved in the reaction?

e). what is H for the above reaction in kJ/mol.

Explanation / Answer

the balanced reaction is HCl + NaOH-------.NaCl + H2O 1 mole of HCl reacts with 1 mole of NaOH to give 1 mole of NaCl and 1 mole of water.

moles= molarity* Volume (L)

moles of HCl reacted = moles of NaOH reacted = 1*50/1000= 0.05

since ther is temperature rise during the couse of reaction, the reaction is exothermic.

heat evolved= mass* specific heat* temperature difference =

volume of solution =100ml, density =1 g/ml, mass of solution =100*1=100gm

heat evolved in cal = 100*1*(31.5-25)= 650 cal

heat evolved /mole= 650/0.05=13000 Cal/mole

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