15.A 0.200 L solution of .950M hydrochloric acid is used to neutralize a 10.0 g sample of calcium hydroxide in a coffee-cup calorimeter. Calcium hydroxide solution is known as slaked lime and is used in agriculture to “sweeten” acidic soils. The temperature in the calorimieter was observed to rise from 20.0*Cto29.2*C during the course of the neutralization. Assume that the density of the hydrochloric acid solution is 1.00g/mL and that the specific heat capacity of the system is the same as that for water,4.18J/g-K.Assume that only the water is available to absorb or release heat and that the reaction is at constant pressure.
2HCI(aq)+Ca(OH)2(aq)------CaCI2(aq)+2H20(I)
a.What was the limiting reagent in the neutralization reaction? Provide support for your answer.
b.How many moles of excess reagent were left over?
c.If 5.1 g of calcium chloride were obtained after the neutralization was complete, what was the percent yield?
d.What was the enthalpy change for the system in the coffee-cup calorimeter?
e.What was the heat of reaction per mole of water produced for the neutrailization reaction?
2006-12-22
10:34:38
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3 answers
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kittyvamptress
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Chemistry