My teacher said to make a Calorimeter lab report on this stuff.
What is the change in enthalpy for magnesium after the reaction with vinegar?
vinegar is 60ml
magnesium is 0.7g
T1 = ?
T2 = 31.8°C
Can someone HELP get started because I really don't know how to start it!
I need help
I don't believe you have enough information to answer this qwuestion. You want to know the enthalpy for Mg AND you want to know the initial T. You CAN calculate dH for Mg from this but you have no data. You can look that information up in your text or ion Google. Call acetic acid HAc, then
Mg + 2HAc ==> Mg(Ac)2 + H2(g)
Look in your tables for dHo formation for HAc and Mg(Ac)2. Then
dHrxn = (n*dHo of products) - (n*dHo of reactants)
That will give you dHo or enthalpy for the reaction pf 1 mol Mg. which is 24.3 g. Convert that to 0.7 g Mg. Let's call that value q,
Then q = mass HAc x specific heat HAc solution x (Tfinal-Tinitial)
You know the value for q. Assuming the density of the HAc solution is the same as water then mass of the solution is 60 grams. Assuming the specific heat is the same as water solution that will be 4184 J/oC*g and you know Tfinal. Solve for Tinitial.
I don't know if this is what you are looking for. The problem I'm having is that you have two unknowns; i.e., you want enthalpy and you want Ti. I am showing yu how to calculate q but that may not be what you want.
To determine the change in enthalpy for the reaction between magnesium and vinegar, you will need to conduct an experiment using a calorimeter. The calorimeter is a device that measures the amount of heat absorbed or released during a chemical reaction. Here's how you can get started on your lab report:
1. Introduction:
Start by introducing the purpose of your experiment, which is to measure the change in enthalpy for the reaction between magnesium and vinegar. Explain that enthalpy is a measure of heat energy transfer in a chemical system.
2. Background information:
Provide some background information about the reaction between magnesium and vinegar. Explain that vinegar is a diluted form of acetic acid (CH3COOH) and that magnesium reacts with the acid to produce hydrogen gas (H2) and magnesium acetate (CH3COOMg). Mention that this reaction is exothermic, meaning it releases heat.
3. Materials and apparatus:
List all the materials and apparatus you used in the experiment. In this case, it would include a calorimeter, 60 mL of vinegar, and 0.7 g of magnesium. You should also mention any safety precautions taken during the experiment.
4. Experimental procedure:
Explain how you conducted the experiment step by step. Here's a suggested procedure:
a. Set up the calorimeter by placing 60 mL of vinegar into it.
b. Weigh out 0.7 g of magnesium.
c. Record the initial temperature of the vinegar in the calorimeter (T1).
d. Add the magnesium to the vinegar and quickly cover the calorimeter.
e. Stir the mixture gently and continuously while monitoring the temperature.
f. Record the highest temperature reached by the mixture (T2).
5. Data analysis:
Calculate the change in temperature (∆T) by subtracting the initial temperature (T1) from the final temperature (T2). In this case, ∆T = T2 - T1.
6. Calculation of enthalpy change:
Using the mass of magnesium, you can calculate the heat energy released during the reaction. The equation for this calculation is: q (heat energy) = mass (magnesium) × specific heat capacity (water) × ∆T.
7. Results and discussion:
Present your experimental data, including the initial and final temperature, as well as the change in temperature (∆T). Calculate the heat energy released during the reaction (q) based on the mass of magnesium used. Then, discuss the significance of your findings, including any sources of error and possible improvements for future experiments.
8. Conclusion:
Summarize your findings and state the change in enthalpy for the reaction between magnesium and vinegar based on your experimental results.