Docsity
Docsity

Prepare for your exams
Prepare for your exams

Study with the several resources on Docsity


Earn points to download
Earn points to download

Earn points by helping other students or get them with a premium plan


Guidelines and tips
Guidelines and tips

Lab Report: Calorimetry and Hess’s Law, Lab Reports of Chemistry

Metal + HCl Reaction and Metal Oxide + HCl Reaction consist of experimental data, data analysis,

Typology: Lab Reports

2020/2021

Uploaded on 05/11/2021

marylen
marylen 🇺🇸

4.6

(26)

250 documents

1 / 4

Toggle sidebar

This page cannot be seen from the preview

Don't miss anything!

bg1
Santa Monica College Chemistry 11
Calorimetry and Hess’s Law Page 1 of 4
Name: Date:
Lab Partner: Lab Section:
Lab Report: Calorimetry and Hess’s Law
Metal + HCl Reaction
Experimental Data
Assigned Metal:
Trial 1 Trial 2
Mass of dry, empty calorimeter
Mass of calorimeter plus HCl
Mass of HCl used
Mass of dry, empty beaker
Mass of beaker plus metal
Mass of metal used
Initial (equilibrium) temperature of HCl
Final (maximum) temperature of mixture
Data Analysis
1) Write the balanced equation for the reaction between your assigned metal and HCl. All
balancing coefficients should be whole numbers.
2) Complete the table below with the results of your calculations.
Trial 1 Trial 2
Total mass of mixture, m
Temperature change of mixture,
T
SHC of mixture, c (use SHC of water)
Heat absorbed by mixture, in J
Heat released by reaction, in J
Hrxn in J/g of metal used
Hrxn in kJ/mol of metal used
Hrxn in kJ for the rxn as balanced in (1)
Average
Hrxn in kJ
pf3
pf4

Partial preview of the text

Download Lab Report: Calorimetry and Hess’s Law and more Lab Reports Chemistry in PDF only on Docsity!

Name: Date: Lab Partner: Lab Section:

Lab Report: Calorimetry and Hess’s Law

Metal + HCl Reaction

Experimental Data

Assigned Metal: Trial 1 Trial 2 Mass of dry, empty calorimeter Mass of calorimeter plus HCl Mass of HCl used Mass of dry, empty beaker Mass of beaker plus metal Mass of metal used Initial (equilibrium) temperature of HCl Final (maximum) temperature of mixture

Data Analysis

  1. Write the balanced equation for the reaction between your assigned metal and HCl. All balancing coefficients should be whole numbers.

  2. Complete the table below with the results of your calculations. Trial 1 Trial 2 Total mass of mixture, m

Temperature change of mixture, ∆ T

SHC of mixture, c (use SHC of water) Heat absorbed by mixture, in J Heat released by reaction, in J

∆ Hrxn in J/g of metal used

∆ Hrxn in kJ/mol of metal used

∆ Hrxn in kJ for the rxn as balanced in (1)

Average ∆ Hrxn in kJ

  1. Show your work for the following calculations using your Trial 1 data only:
  • Heat absorbed by mixture, in J
  • Heat released by reaction, in J
  • Hrxn in J/g of metal used
  • Hrxn in kJ/mol of metal used
  • Hrxn in kJ for reaction as balanced in (1)
  1. Is this reaction exothermic or endothermic? What is your experimental evidence supporting

this? Is ∆ Hrxn positive or negative?

Enthalpy of Combustion of a Metal

  1. Write the balanced equation for the combustion of your assigned metal. All balancing coefficients should be whole numbers.

  2. Using Hess’s Law, determine the enthalpy of combustion of your assigned metal as balanced above. To do this, you will need the balanced thermochemical equations for the two reactions studied in this lab, plus the balanced thermochemical equation for the formation of water from its elements. Clearly show how these three equations (and their reaction enthalpies) must be combined to give the target combustion reaction.

  3. Calculate the theoretical value for the enthalpy of combustion of your assigned metal, using

the tabulated ∆ Hf ° values from the text.

  1. Determine the percent error in your experimentally determined value for the enthalpy of combustion.