A 106.2 mL sample of 1.00 M NaOH is mixed with 53.1 mL of 1.00 M...

A 106.2 mL sample of 1.00 M NaOH is mixed with 53.1 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 21.65 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 31.50 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g·°C), and that no heat is lost to the surroundings.

Expert Solution

2NaOH(aq) + H2SO4(aq) --------------> Na2So4(aq) + 2H2O(l)

no of moles of NaOH = molarity * volume in L

= 1*0.1062 = 0.1062moles

no of moles of H2So4 = molarity * volume in L

= 1*0.0531 = 0.0531moles

Total volume of solution = 106.2 + 53.1 = 159.3ml

mass of solution = volume of solution * density

= 159.3*1 = 159.3g

q = mcT

= 159.3*4.18*(31.5-21.65) =- 6559J

H = -6559J = -6.559KJ

= -6.559KJ/0.1062mole = -61.76KJ/mole >>>>answer

queen_honey_blossom answered 2 years ago

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