Preview

Ib Chemistry Sl Enthalpy Design Lab

Good Essays
Open Document
Open Document
536 Words
Grammar
Grammar
Plagiarism
Plagiarism
Writing
Writing
Score
Score
Ib Chemistry Sl Enthalpy Design Lab
Chemistry SL Internal Assessment: Enthalpy Change Design Lab
Experiment: Reaction of distilled water and solid sodium hydroxide
RESEARCH QUESTION
How does the heat released during the reaction between distilled water and Group 1 elements (lithium, sodium and potassium) vary as one goes down the group?
OBJECTIVE
The objective of the experiment is to measure the heat change during the reactions with minimal heat loss to the surroundings.
MATERIALS
The materials to be used in this experiment are:
Lithium, sodium, and potassium metal are the three Group 1 elements and reactants.
• Distilled water is a reactant.
• 250ml beaker to measure the water.
• Polystyrene cup to hold the water.
• Knife to cut the metals.
• Digital balance to measure the mass of the metals.
• Calorimeter to trap the heat during the reactions.
• Thermometer to measure the initial and final temperatures during the reaction.
• Paper and pencil to record data such as masses and temperatures.
• Lab coat and goggles for safety.
VARIABLES
• Dependent: Temperature
• Independent: Type of substance
CONTROL VARIABLE
• The mass of the substance is the control variable, since there is a fixed amount of substance being used in the reaction to control the rate of reaction.
UNCERTAINTIES
• Temperature: There is an uncertainty of ± 0.1 oC since the calorimeter is not closed at all times and there can be inaccuracies in the thermometer.
• Mass: There is an uncertainty of ± 0.1 g due to inaccuracy of the digital balance.
PROCEDURE
o Lithium

• Cut out a small piece of lithium metal.
• Measure about 2g of lithium on a digital balance and place it in a beaker.
• Measure about 100 ml (100 g) of distilled water in a 250 ml beaker.
• Use a thermometer to measure the temperature of the water.
• Pour the water into a polystyrene cup and place it in a calorimeter.
• Add lithium to the water.
• Allow the reaction to occur and then measure the temperature.

o Sodium

• Cut out a small

You May Also Find These Documents Helpful

  • Powerful Essays

    1. Place 3 grams of Salicylic acid in a Erlenmeyer flask and record the mass…

    • 1900 Words
    • 8 Pages
    Powerful Essays
  • Good Essays

    Controlled: the same type of beaker as the mass of the beaker is never changed…

    • 951 Words
    • 4 Pages
    Good Essays
  • Better Essays

    Background: Calorimetry is the science of measuring the heat of chemical reactions or physical changes. Calorimetry is performed with a calorimeter. A calorimeter can be any container from a cup to a Calorimeters need to be well insulated as calorimetry relies on the fact that temperature change only occurs within the solution and that no heat escapes to the surroundings. That is why it is important that calorimeters are well insulated. However, heat loss cannot be avoided so scientists, when conducting experiments, need to choose the calorimeter that allows least heat energy to escape, therefore, retaining as much heat within the solution…

    • 2565 Words
    • 11 Pages
    Better Essays
  • Good Essays

    A calorimeter is to be arranged using Styrofoam cups and a hole on top of a cover to take the temperature while also preventing heat loss. 50mls of distilled is to be added to the calorimeter. 75mls must then be heated to 70 degrees Celsius and 50mls of that water is to be added to the calorimeter. The calorimeter has to be covered and then the temperature taken every 20 seconds for 3 minutes.…

    • 1075 Words
    • 5 Pages
    Good Essays
  • Good Essays

    Determination of Enthalpy

    • 1206 Words
    • 5 Pages

    In this experiment, you will measure the temperature change of two reactions, and use Hess’s law to determine the enthalpy change, ΔH of a third reaction. You will use a Styrofoam cup nested in a beaker as a calorimeter, as shown in Figure 1. For purposes of this experiment, you may assume that the heat loss to the calorimeter and the surrounding air is negligible.…

    • 1206 Words
    • 5 Pages
    Good Essays
  • Powerful Essays

    Calorimetry Chemistry Lab

    • 971 Words
    • 4 Pages

    To determine the specific heat of an unknown metal through the use of a calorimeter.…

    • 971 Words
    • 4 Pages
    Powerful Essays
  • Good Essays

    What is the overall conductance (UA) for this exchanger under the experimental conditions described above?…

    • 505 Words
    • 3 Pages
    Good Essays
  • Better Essays

    Potato Cores Lab

    • 2661 Words
    • 11 Pages

    Measured before putting the pieces into the solutions with a ruler (in mm) and an electronic balance (in gram).…

    • 2661 Words
    • 11 Pages
    Better Essays
  • Powerful Essays

    E  0  qsystem  qsurroundings  qcalorimeter In the first portion of our experiment, a known mass of water with a known temperature will be used to determine how much energy is being absorbed by the calorimeter. Once this is known, the change in enthalpy from the decomposition of hydrogen peroxide can be determined. 2H2O2(aq)  2H2O(l) + O2(g) A solution of hydrogen peroxide will be added to the calorimeter and its temperature will be monitored for a short time. A small amount of iron nitrate will be added to catalyze the reaction and produce a measureable temperature change. This temperature change will be plotted over time. Using this plot, the mass of solution, its specific heat, the calorimeter constant, and the temperature change, we will be able to determine the enthalpy…

    • 1439 Words
    • 6 Pages
    Powerful Essays
  • Good Essays

    Enthalpy Lab Background

    • 751 Words
    • 4 Pages

    Enthalpy, represented by the sign ∆H in kJ/mol, is the heat change in a reaction. It shows whether how much heat is released or absorbed during the reaction. If the reaction is endothermic, the enthalpy would be positive and if the reaction is exothermic, the enthalpy would be negative. During a chemical reaction, which consists of breaking and creating bonds, heat is either absorbed or released. In this lab, the reaction uses the disassociation of an ionic compound ammonium nitrate shown in the equation #1 below into ions. In order to disassociate ammonium nitrate into ions, energy is required. Both NH4 and NO3 are always soluble, therefore the ionic compound disassociates completely. Through equation #2, heat absorbed or released can be measured. In equation #2, q stands for the heat change in joules, m for the mass of the water in grams, C for the specific heat of water, and ∆T for the change in temperature. By using the calorimeter with a stir rod, change in temperature is found.…

    • 751 Words
    • 4 Pages
    Good Essays
  • Better Essays

    During the experiment, it was observed that heat was both gained and lost. The hot water lost 2,853.95 Joules (J) while the tap water gained 2,472.74 Joules (J). In general, the calorimeter has a heat capacity of 25.414 J/°C. All the data that was recorded is shown in Table 1.…

    • 2511 Words
    • 11 Pages
    Better Essays
  • Good Essays

    Hess’ Law, which says that the heat of configuration (enthalpy change, ΔH) of a reaction can be compute by taking away the ΔH of the products from the ΔH of the reactants, is illustrated through this lab experiment.…

    • 367 Words
    • 2 Pages
    Good Essays
  • Good Essays

    Calorimetry Experiment

    • 410 Words
    • 2 Pages

    I was able to conclude that my calorimetric constant for this calorimeter is 95J/g C.…

    • 410 Words
    • 2 Pages
    Good Essays
  • Satisfactory Essays

    Osmosis experiment

    • 411 Words
    • 2 Pages

    Independent variables are the different solutions of sucrose, the dependent variable is the change in mass, and the controlled variables include the volume of liquid, the length of each piece, where the test tubes are kept and the time each piece had in each test tube.…

    • 411 Words
    • 2 Pages
    Satisfactory Essays
  • Good Essays

    If the reaction produces heat (increases the temperature of the surroundings) then it’s exothermic. If it decreases the temp (i.e. absorbs heat) then it’s endothermic. Also, the yield of an equilibrium reaction which is exothermic will be increased if it occurs at low temps, and so for endothermic reactions at high temperatures.…

    • 1224 Words
    • 5 Pages
    Good Essays

Related Topics