A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 ml_ of 1.00 M H_2SO_4 in a l

Question

A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 ml_ of 1.00 M H_2SO_4 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 23.7^degree C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.1 ^degree 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- ^degree C), and that no heat is lost to the surroundings. Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Is any NaOH or H_2SO_4 left in the Styrofoam cup when the reaction is over? Type an open parenthesis "(" to add a phase. Phases should not be subscripted. Use the left and right arrow keys to move the cursor out of a superscript or subscript in the module. Include phases in the balanced chemical Calculate the enthalpy change per mole of H_2SO_4 in the reaction.

Explanation / Answer

a) H2SO4 (aq) + 2NaOH(aq) = Na2SO4 (aq) + 2H2O (l)

b) No

c) Q = mS*delta T

Her m = volume *density = (100+50)*1 = 150gms

Q = 150*4.18*(30.1-23.7) = 4012.8 J = 4.0128 KJ

Moles of H2SO4 = 50*10^-3*1 = 0.05

Change of enthalpy per mole of H2SO4 = 4.0128 / 0.05 = 80.256 KJ/mol

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