Sodium Bicarbonate Decomposition

Sodium bicarbonate has a molar mass of 84.0 g/mol. It has a melting point of 50°C and can be an irritant.

Aspirin Recrysalization Data Table Actual Mass (g) 0.41 Actual MP (ºC) 123-125 Expected Mass (g) 0.533 Expected MP (ºC) 135 Percent Recovery 77% Percent Error 8%

The powdered cobalt oxalate hydrate was weighed to about 0.3 g and placed in a pre-weighed crucible. The crucible and the cobalt oxalate were then heated until the cobalt oxalate decomposed into a stable, black solid, or Co3O4. Once the crucible was sufficiently

Suppose a household product label says it contains NaHCO3. How would you test this material for the presence of sodium bicarbonate?

Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next

Used stirring rods to completely remove copper from that wire. And then completed the removal of copper using 5 drops of 6M HCl, adding it onto copper. There will produced copper in a solution. Connected Buchner flask to the vacuum line and place filter paper in it to completely washed off the copper. Then, add 95% ethanol to copper and leave it for 1 min and turned section back for 5 mins. Measured mass of clean, dry watch glass. Transfer copper to watch glass and dry it under heat lamp for 20 mins, allowed it to cool to room temperature and then accurately determine its mass.

First I will set up the apparatus as show above. I will add 1.5 grams

Materials:Magnesium stripCrucibleCrucible coverClay triangleIron ringRetort standTongsBalanceBunsen burnerProcedure:1.obtained a strip of magnesium between 30-40 cm long2.coiled magnesium strip into a tight roll3.measured the mass of the crucible and cover4.Added the magnesium strip to the crucible and measured the

2. Summarize the following description of a chemical reaction in the form of a balanced chemical equation?

The mixture was heated at 120°C using an aluminum block and was stirred gently. After all of the solid dissolved, it was heated for 20 additional minutes to ensure the reaction was complete.

* By using the dropper and measuring cylinder, 7 ml sodium carbonate solution was added to the test tube

Experiment was followed as stated in CHEM 2420 Experiments in Organic Chemistry from the University of Wyoming, written by Dr. Ed Clennan and edited by Malgorzata M. Clennan. However, the following deviations were made. In step 5c, 0.74 grams of boiling stones were added. In step 6, the heat was set to medium and was turned higher as the experiment progressed.

Stoichiometry has many uses in the real world. In the chemical industry and in professional scientific experiments, scientists use stoichiometry to save money. Scientists use stoichiometric calculations to determine the amount of a substance they need to purchase for a specific reaction. There are four possible reactions that can occur when sodium bicarbonate thermally decomposes. In this lab, stoichiometry was used to find out which balanced chemical equation out the four best represents the thermal decomposition of sodium bicarbonate.

The materials used for the project are 9 cups of sugar, ⅓ cup citric acid, 4 cups of waters. My procedure for the project was I boiled 9 cups of sugar, and 2 cups of water, after 15 minutes I put half of the sugar water in one pot and the other half in another pot. In one pot I added ⅓ cup of citric acid into it, transforming it

All ammonium compounds, which contain an ammonium ion (NH4+) and a negative ion, are thermally unstable. A. Discuss two ways that ammonium compounds decompose when they are heated. What chemical reaction is involved in the thermal decomposition of ammonium persulfate? The ammonium ion is known for exhibiting unique thermal decomposition reactions when heated because "there are a considerable number of stable crystalline salts of the ammonium ion [14798-03-9] NH+4" (Clintern, 2007). Ammonium acetates emit toxic ammonia fumes when heated, while ammonium bicarbonate "decomposes below its melting point, dissociating into ammonia, carbon dioxide, and water" (Clintern, 2007). There are some ammonium salts, such as ammonium dichromate, ammonium permanganate, ammonium nitrate, and ammonium nitrite, which undergo an oxidation-reduction reaction after being heated: