Acetic Air Lab

The purpose of the lab was to determine the ratio of air to acetylene results in complete combustion of acetylene gas. The balanced chemical equation for this experiment was C2H2(g) + O2(g) --> CO2(g)+ H2O(l). Complete combustion is the reaction of an element or compound with oxygen to produce the most common oxides and energy. Complete combustion occurs when the fuel and oxygen combine in exact proportions to completely burn the fuel, which leaves a clean test tube. Incomplete combustion is the reaction of an element or compound with oxygen to produce some oxides with less oxygen than the most common oxides. Incomplete combustion occurs when there is not enough oxygen to react

The vials were placed in the water and the oxygen levels were read every 5 minutes until 30 minutes was reached. As the oxygen levels were collected they were put into a table that had all three tubes labeled at each 5-minute increment. After 30 minutes the experiment was completed and the clean up process could begin.

To performed the experiment, a volumeter was set up to measure the net oxygen production under white light, then a second step was followed to measure oxygen consumption under dark conditions (oxygen production only happens in the presence of light and oxygen consumption in the presence of dark light) and finally, a third step consisted of recording the measure of the net oxygen production under the presence of green light.

Please Note: This lab involves a lot of waiting for the gas collection. Make sure you allot yourself the full three hours to perform the experiments.

The purpose of this experiment was to simply measure oxygen production rates released from decomposed hydrogen peroxide under different conditions (concentration of enzymes, temperature, and PH level).

This lab will be driven by the research question, what is the effect of temperature (at 5oC, 15oC, 25oC, 35oC and 45oC) on the photosynthetic rate (measure of oxygen bubbles over a period of time) of Elodea (pondweed)?

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

-The more dissolved oxygen in the water, the more fish is observed in that area of water.

a) Tap and drag over the area of the graph where the resting heart rate is displayed to select the data.

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

Purchase gallon containers of spring water and distilled water at the local supermarket. Using the dissolved oxygen probe, measure the initial dissolved oxygen concentration before the water has been removed from the original container.

However, because the deviation between the oxygen and ideal gas behaviors are very small in the experiment environment and thus can be ignored. So, the ideal gas equation PV=nRT can be used to determine the mole of oxygen generated. Equipment & Reagents Equipment: graduated flask, test tube, alcohol burner, pipette, rubber catheter, glass catheter, glass flume, iron support, dispensing spoon, match, balance, weighing paper. Reagents: KClO_3, MnO_2; (Potassium chlorate, Manganese

The 1,000ml graduated cylinder was held secure in the tub as the gas started to push the water down. Occasionally, the Erlenmeyer flask would be stirred to ensure that the reactants combined. After the reaction was completed, changes to the amount of water in the 1,000ml graduated cylinder was

By using a catalyst to break down the Hydrogen Dioxide into oxygen and water, my partner and I were able to determine the molar volume of oxygen from the volume we produced in the experiment. The chemical equation for the reaction was:

When all the materials were gathered. The measurements were made. Though while getting the measurements, the AC vent was above the lab and had a affected the weight of the scale, which had caused the measurements to little bit off. With the recipients in the beaker, the next step was to cut the filter paper to fit into the Buchner Funnel, while it took some time to get it to fit into the funnel and then get the weight. One of the next mistakes takes place as we poured the mixture into the beaker. We intended to pour slowly but by the time we tilted the beaker it was to late, some of the product had already passed the filter and went into the the filter flask. How we had noticed this is that the liquid that had passed through the filter was very yellow, it was supposed to be mostly clear. Since we