Baria Chloride Lab

6-3: This process is used by cells to manufacture _biochemical energy from nutrients into adenosine triphosphate (ATP), and then release waste products__

Sodium Bicarbonate (also known as baking soda) is something used everyday. Baking soda is a very common ingredient in cooking- one of its main uses is to make cakes "risk" due to the compounds produced. (Summer Chemistry Workshop). The lab was to use decomposition, the chemical change in which a single compound breaks down into two or more simpler products (Pearson Chemistry, 358), listed below are the possible reactions.

5. I believe that with a Bunsen burner to dry would have provided more accurate results for the hydration number because the heat can be applied more directly and the time to heat would be faster, giving less room for error in the

What is the percentage yield of the reaction of iron and copper chloride when steel wool and copper chloride dehydrate are used as reactions?

Day 1. Michael was coming home for vacation from college. When he got home he found out that

Substances A and B have an appearance of a white solid like. Substances A and B were put into a test tube and on the Bunsen burner. As a result, B melted faster than A. A was slow to melt. The reason why B melted faster than A is because it has a lower boiling point than substance A which made it melt faster. It also shows that A needs more energy than B to be broken down.

3.6.1. BAP (Benzyl amino purine) stock solution (2mg/ml): 20mg of BAP being weighed and dissolved completely in 1N NaOH to a final total volume of 10 ml with autoclaved double distilled water to obtain a stock concentration of 2mg/ml was prepared and stored in clean autoclaved vials at -4°C.

1. Place a small amount of wax from a birthday candle into a test tube. Heat gently over a burner flame until the wax melts completely; then allow

In experiment 3.11, we found out whether or not a larger amount of a liquid would get hotter when it boils. To answer this, we heated a specific amount of unknown liquid and recorded the temperature every fifteen seconds. In our scatter plot, we were able to find the boiling point of our liquid. We know that the slope of our graphs is when the liquid molecules were moving around and heating up. The plateau of our graph points is where the liquid started to evaporate and boil. This is were we found our boiling point at. Shantel and I decided that our boiling point was about 98º Celsius. If you had another slope in your graph, that was when you were simply heating the leftover gas. The histogram showed us that there were about equal amounts of data in the higher temperature (about 95º Celsius) bins for both 20mL of liquid and 10mL of liquid. Also, in the lower temperature bins (75º to 80º Celsius) there was about equal amount of data for 20mL of liquid and 10mL of liquid. There was 7 pieces of data for 10mL of liquid in the lower bins, and 6 pieces of data for 20mL of liquid. If a larger amount of liquid did have a higher boiling point, the clusters would be organized by volumes or amount. For example, all of the 20mL pieces of data would be in the higher temperature bins, and all of the 10mL pieces of data would be in the lower temperature bins or flipped. Rather, the bins were clustered by identity. The boiling point is a characteristic property.

4. Allow the crucible to cool with the lid on. When cool, determine the mass of the crucible and lid with the dehydrated compound. 5. Examine and describe the anhydrous compound in the crucible.

Fill the crucible halfway with the unknown hydrate. Measure and record the mass of the crucible and the hydrate.

The cooling time caused error when calculating the moles of water because the actual result was seven moles instead of five moles which was what was calculated. The calculations could have been potentially miscalculated particularly due to the significant figures used in the data. The method for this experiment can be improved by maybe using another object rather than the crucible to allow a faster cooling time that way the calculations for the analysis have less of a chance of

To start your experiment you need to get all your materials. You will need,three cups, three shells, acid, measuring spoons, electronic balance and water. First we're gonna pour 120 ml (water) in the three cups ( tps whole ⅛ ). Then were gonna put one shell in each cup and let them soak in the acid. Then we're gonna take them out and measure the different weight. Cup A will need a whole tps and the rest filled with water. Cup B is gonna need ¼ tps and the rest filled with water. Cup C will need ½ tps and the rest water. gonna need

BTB or Bromothymol blue, is a liquid is mixed with oxygen If BTB is yellow, there is no oxygen in the matter. Yellow is less acidic and Blue is basic. The colors in the process are blue, then green, and finally yellow. The whole purpose of this BTB experiment was to find out if the water plants give out in the light. Would they also give oxygen in the dark? And or if the matter does not matter if the plant is in the dark or in the light. The guiding questions was, do they give light off? Do they use it? Could they possibly do both? Does it matter whether they are in the light or in the dark? My predictions were that the plants would give oxygen when there is blue BTB in the sun. If yellow BTB, no change in color. If there was no sunlight for the plants, the liquid

Firstly, after removed from the Bunsen burner, the crucible was not given time to cool down before being weighed. Weighing a hot crucible can affect the accuracy of measurements by making the crucible appear to weigh heavier, causing the results to be overstated. Secondly, as state in the paragraph above, both samples did not weigh exactly 2g. In trial 1, the sample weighed slightly less than 2g but in trial 2 the sample weighed slightly more than 2g. Consequently, the net weight for the solid in trial 1 was understated and the net weight for the solid in trial 2 was slightly