# Calorimetry and Hess’s Law Purpose

Published: 2021-07-24 15:40:06  Category: Physics, Chemistry, Thermodynamics, Heat

Type of paper: Essay

This essay has been submitted by a student. This is not an example of the work written by our professional essay writers.

Hey! We can write a custom essay for you.

All possible types of assignments. Written by academics

GET MY ESSAY The purpose of this lab is to determine the enthalpy of reaction for the burning of one mole of magnesium in oxygen. Although the reaction is exothermic, the ∆HRXN will be determined by using calorimetry and then using Hess’s Law to manipulate the data collected to yield the answer needed.
Part A

Haven’t found the relevant content?
Hire a subject expert to help you with Calorimetry and Hess’s Law Purpose

Hire verified expert

Volume of cold water
49. 9 mL

Temperature of cold water (in a cup)
23. 50 C

Volume of hot water
49. 9 mL

Temperature of hot water (in a cup)
550 C

Calculations

Mass of cold water
49. 9 g

Tf from the graph by extrapolation
34. 90 C

∆THW for hot water
-20. 1

∆TCW for cold water
11. 4

qHW for hot water
-4196. 5 J

qcw for cold water
2380. 1 J

qCal for the cup
1816. 4 J

Ccup for the cup
159. 3 J

Part B

Description of sample
Metal fizzed when dissolved in HCl

Volume of HCl
100 mL

Initial Temperature
220 C

Mass of Mg
0. 1485 g

Calculations

Tf from graph
50 C

Mass of HCl
100 g

∆TCW for HCl
-2092 J

qHCl for solution
-204. 4 J

qCal for cup
-2296. 4 J

qRXN
-47594 J

∆HRXN for Mg
-

NET REACTION: 2HCl(aq) + Mg(s)>MgCl2(aq) + H2(g)
Part C

Description of sample
-

Volume of HCl
100 mL

Temperature of HCl
220 C

Mass of MgO
0. 5052 g

Calculations

Tf from graph
240 C

∆TCW for HCl
1. 50 C

qHCl for HCl
627. 6 J

qCal for cup
61. 32 J

qRXN
608. 92 J

∆HRXN for Mgo
55469 J/mol

Net Equation: 2HCl(aq) + MgO(s)>MgCl2(aq) + H2O(l)
Conclusion
In this experiment, we had to find the heat capacity of the calorimeter cup using two trials of hot and cold water. When we obtained the data after 10 minutes of recording 30-second intervals of the calorimeter cup temperature, we created a line graph to show the trend line.
With the trend line, we could figure out the final temperature and delta H in the process. With the equation we could find the heat of reaction for hot water q HW = m c DTHW and using qCW = m c DTCW we could find the heat of reaction for cold water. By using |qHW| = |qCW |+ qCal, we can find the heat of reaction of the cup and multiply that by the change in temperature to find the heat capacity. After placing Mg into HCl and then the same thing with MgO, we could find the heat of solution of HCl with q CW = m c DTHCl.
When we found the values of DHRXN for B and C we can use Hess's Law, which is shown in the calculations section. All the data is in the data section of the report. The percent error of Mg was about 30%. The actual value of Mg was 601200 J/mol and the experiment we obtained was 420611 J/mol. There could have been human error in order to obtain the results that could have accounted for the 30% error, although this is not so high. Also, the heat of formation we used was MgO(s) for the actual value, although in the experiment it was a gas. This could have also accounted for some errors.
References:

“ Calorimetry and Hess’s Law. ” Laboratory Manual. Publishing, 2012, pp. 168-177.

#### Warning! This essay is not original. Get 100% unique essay within 45 seconds!

GET UNIQUE ESSAY

We can write your paper just for 11.99\$

i want to copy...

This essay has been submitted by a student and contain not unique content