Evaporation Vs Calorimetry Essay
My hypothesis is that if I turn the water to vapor then I will be able to determine the ratio and the amount of moles of the salt and water. This is because by using evaporation I will be able to learn the mass of the salt and of the water needed for n=m/MM which states the amount of moles can be found by dividing mass of the moles by the molar mass.
Experiment 1
First I took a crucible, a balance, and a Bunsen burner and placed them onto the workbench.
Then I measured the mass of the empty crucible with the balance and recorded it in my notes.
Next I added 5 g of the copper sulfate hydrate to the crucible.
I measured the mass of the crucible with the balance and recorded it in my notes.
Then I moved the crucible onto the Bunsen burner and
set it on medium flame.
I waited 2 minutes for all of the water to be released as vapor and then waited for it to cool off.
After cooling off, I measured the mass of the crucible with the balance and recorded it in my notes.
Experiment 2
It was exactly the same as experiment 1, except I used magnesium chloride hydrate instead of copper sulfate hydrate.
My hypothesis was correct. By using evaporation I was able to gain the mass of the MgCl2 and CuSO4 ( 2.342 g and 3.196 g respectivly) which in turn allowed me to find how many moles they had (0.025 and 0.020) and thier ratio with water (1:5 and 1:6). This was however expected as according to the equation n=m/MM, all you need to find the amount of moles (and thus thier ratio with H2O) is thier mass in the compound and also thier molar mass information. This conclusion also shows that to properly determine the mass of elements in a compound, the hydrate will need to be decomposed (such as I did by using the Bunsen burner).If I were to redo this experiment, I would use a non salt along with a salt in order to have greater diversity in the different compounds that I decompose. Ultimately this was a great experiment that shows that via decomposing, we can measure needed values in order to gain correct calculations.
Experiment 1
First I took a crucible, a balance, and a Bunsen burner and placed them onto the workbench.
Then I measured the mass of the empty crucible with the balance and recorded it in my notes.
Next I added 5 g of the copper sulfate hydrate to the crucible.
I measured the mass of the crucible with the balance and recorded it in my notes.
Then I moved the crucible onto the Bunsen burner and
set it on medium flame.
I waited 2 minutes for all of the water to be released as vapor and then waited for it to cool off.
After cooling off, I measured the mass of the crucible with the balance and recorded it in my notes.
Experiment 2
It was exactly the same as experiment 1, except I used magnesium chloride hydrate instead of copper sulfate hydrate.
My hypothesis was correct. By using evaporation I was able to gain the mass of the MgCl2 and CuSO4 ( 2.342 g and 3.196 g respectivly) which in turn allowed me to find how many moles they had (0.025 and 0.020) and thier ratio with water (1:5 and 1:6). This was however expected as according to the equation n=m/MM, all you need to find the amount of moles (and thus thier ratio with H2O) is thier mass in the compound and also thier molar mass information. This conclusion also shows that to properly determine the mass of elements in a compound, the hydrate will need to be decomposed (such as I did by using the Bunsen burner).If I were to redo this experiment, I would use a non salt along with a salt in order to have greater diversity in the different compounds that I decompose. Ultimately this was a great experiment that shows that via decomposing, we can measure needed values in order to gain correct calculations.