A 73.0 mL sample of 1.0 M NaOH is mixed with 43.0 mL of 1.0 M H2SO4 in a large S

Question

A 73.0 mL sample of 1.0 M NaOH is mixed with 43.0 mL of 1.0 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 21.8 degree C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. 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 middot degree C), and that no heat is lost to the surroundings. The DeltaHrxn for the neutralization of NaOH with H2SO4 is -114 kJ/mol H2SO4. What is the maximum measured temperature in the Styrofoam cup?

Explanation / Answer

0.043L * 2moles NaOH/mole H2SO4 = 0.086 moles of NaOH required 0.073L * 1mol/L = 0.073 moles NaOH available; NaOH limiting 0.073 moles of NaOH is neutralied; 0.073/2 = 0.0365 moles of H2SO4 neutralized. 0.0365 moles * 114 kJ/mole = q = 4.161 kJ = 4164 Joules V = m = 73 + 43 = 116 grams 116 g * 4.18 J/gC * (delta)T = 4164 Joules (delta)T = 4164/(116*4.18) C = 8.59C 21.8C (initial) + 8.59C = 30.4 C Tfinal = 30.4 C

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