Homework Help: Chemistry

Posted by Chen on Sunday, November 6, 2011 at 9:54pm.

A student conducts an experiment to determine the enthalpy of neutralization for phosphoric acid
reacting with sodium hydroxide. The student combines 25.0 mL of equimolar solutions of acid and
base, both having an initial temperature of 22.5 °C, in an open polystyrene calorimeter. Each
solution has a density of 1.00 g/mL and a specific heat of 4.18
J
g • °C
. The student collects data until
a maximum temperature of 26.4 °C is reached.
(a) What assumption is the student allowed to make?
(b) Explain how the student knows data collection is complete.
(c) Calculate the qrxn for the neutralization reaction.
(d) Is the reaction exothermic or endothermic? Justify your answer.
(e) Calculate the ΔHneut
if the initial molarities of both solutions is equal to 0.80 M. Be sure to
report your answer with the correct sign and units.

Chemistry - DrBob222, Sunday, November 6, 2011 at 11:20pm
a) no loss of heat to the surroundings.
b) when the temperature of the solution stops rising.
c) qrxn = mass 50 mL H2O x specific heat x (Tfinal-Tinitial)
d) T rose so rxn must be exothermic.
e) Determine the limiting reagent. DHneut = q/mols
Chemistry - Anonymous, Tuesday, December 4, 2012 at 9:20pm
efw

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