{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

heat of neutralization lab report

heat of neutralization lab report - Kris Kelly Heat of...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
Kris Kelly Heat of Neutralization Lab Report CHEM 121L 12/4/07 Background/Theory: In this experiment, a calorimeter will be used to measure the heat of a reaction between a base and two different acids. A calorimeter is a device used to complete reactions in a controlled environment, where a thermometer is used to determine the heat gained or lost by various pieces of the reaction. In this case, Styrofoam cups with a plastic lid, rubber stopper, and thermometer will be used. Key Data: See attached graphs Sample Calculations: Part A Heat lost by warm water (temperature decrease)(50.0g)(4.18 J/g-k) (13.4 K)(50.0 g)(4.18 J/g-k) 2800.6 J Heat Capacity of Calorimeter (Heat gained by calorimeter)/(temperature increase) (188.1 J)/(14.3 K) 13.15 J/K Part B The number of moles of HCl in 50 ml of 1.0 M HCl Molarity = # of moles / liters of solution 1.0M = # of moles / .05 L # moles = .05 moles HCl in 1.0 M HCl The number of moles of H O produced in reaction of 50 mL 1.0 M HCl and 50 mL 1.0 M NaOH .05 mol HCl x 1 mol H O / 1 mol HCl .05 mol H O
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
.05 mol NaOH x 1 mol H O / 1 mol NaOH .05 mol H O .05 mol H O from HCl + .05 mol H O from NaOH = .10 mol H O
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}