Enthalpy of a Reaction

# Enthalpy of a Reaction - we had exothermic energy given off...

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

Enthalpy of a Reaction Shawn Whitcraft Group Member: Marc Whetstone

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

View Full Document
Statement of Purpose: The purpose of this experiment is to use a calorimeter to measure the amount of energy given off by the reaction of predetermined chemicals. We determine the enthalpy change of the reaction of HCl and NaOH solutions. After measuring the enthalpy change in the first reaction, then we measure the effect of doubling the amount of each chemical in the reaction and record the results. Data Section: Sample Calculations: 1. 2.1g X 50ml (1g/1ml) X 4.18 X 2.8 = 1228.92 4.04g X 50ml (1g/1ml) X 4.18 X 4.4= 3715.184 2. 80 + .2016 X 695 X 2.8 = -156072.3136 3. Q = 100 X 4.18 X 6.8 Q= 2842.4 4. Q=200 X 4.18 X 6.6 Q=5517.6 Results and Discussion: After completing the experiment and completing the calculations, the results showed that when you combine water and ammonium nitrate you will have endothermic energy that can be measured by the decrease in the temperature of the solution. When combining HCl and NaOH,
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: we had exothermic energy given off. This is measured in the rise in the temperature of the solution. When we doubled the amount of ammonium nitrate used in the measurement we had almost had a double in the amount of endothermic energy given off. We noticed a similar result Enthalpy of Reaction Data Chemical One Amount Chemical Two Amount Beginning Temp °C End Temp °C Change °C Test 1 water 50 ml NH 4 NO 3 2.1g 22.8 20-2.8 Test 2 water 50 ml NH 4 NO 3 4.04g 22.8 18.4-4.4 Test 3 HCl 50 ml NaOH 50 ml 22.8 29.6 6.8 Test 4 HCl 50 ml NaOH 100 ml 22.8 26.6 3.8 Test 5 HCl 100 ml NaOH 100 ml 22.8 29.4 6.6 when we doubled the volume of the base and didn’t change the amount of acid. When we doubled the volumes of both the acid and the base, we had similar measurements in exothermic energy as we did before we doubled the two measured amounts of chemicals....
View Full Document

## This note was uploaded on 09/23/2009 for the course POL 101 taught by Professor Staff during the Spring '08 term at Purdue.

### Page1 / 3

Enthalpy of a Reaction - we had exothermic energy given off...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online