a 100 ml sample of 1.00 M Naoh is mixed with 50.0 ml of 1.0 M h2so4 Please answe

Question

a 100 ml sample of 1.00 M Naoh is mixed with 50.0 ml of 1.0 M h2so4
Please answer a, b,and c stion 21 of 23 (1 point) A 100.0-mL sample of 1.00 MNaoH is mixed with 50.0 mL of 1.00 MH2so4 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 adding the NaOH solution to the coffee cup and stirring the mixed the solutions with the thermometer, maximum temperature measured is 31.7 C. Assume that the density of the mixed solutions is 1.00 glmL, that the s heat of the mixed is 4.18 JKg. no heat is lost to the surroundings. (a) write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. (b) Is any NaOH or H2SO4 left in the Include phases in the balanced chemical Styrofoam cup when the reaction is over? equation. Type an open to add a phase. Phases should not be subscripted. Use the left and right arrow keys to move the cursor O Yes out of a superscript or subscript in the module. O No (c) Calculate the enthalpy change per mole of H2SO4 in the reaction. click to edit kJ mol

Explanation / Answer

a) the balnced equation is

2NaOH (aq) + H2SO4(aq) -------> Na2SO4(aq) + H2O (l)

b) milliequivalents of base = 100x 1.0 = 100 meq

milliequivalents of acid = 50x 1.0 x2 = 100meq ( since H2SO4 is dibasic acid)

thus neither acid nor base remains in solution.

c) heat given in neutralization process Q = mass x specific heat x difference in temperature

= 150 g x 4.18J/gx8.2 K

= 5141.4 J

5141.4 J of heat is given by the neutralization of 100 meq of base with 100 meq= 50 moles of acid.

Thus 1000 moles of H2SO4 ca n give heat = 5141.4 x 1000/50

= 102828 J

= 102.828kJ/mol of H2SO4

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