Lithium Lab Report

The objective of this lab was to use prior knowledge about the Law of Conservation of Matter and of different types of chemical reactions in order to evaluate if aluminum disappears during the reaction and copper appears. The reaction that occurred between Copper (II) Chloride and aluminum was a single replacement reaction. Clear signs that a chemical reaction took place include heat release/temperature change, color change, and formation of a precipitate. When a single element, in this instance aluminum, replaces another element in a compound, copper, a single replacement reaction occurs. A basic formula for these reactions is AB + C → AC + B.

An elements¡¦ reaction to certain substances may be predicted by its placement on the Periodic Table of Elements. Across a period, an element on the left will react with more vigor than one on the right, of the same period. Vertically, as elements are sectioned into groups, the reaction of each element increases

There was an increasing trend because the metal was the limiting reactant in this experiment. The amount of each metal placed in the hydrochloric acid was fully used up before the acid was. From Figure 1, it is clear that aluminum produced the most amount of hydrogen gas, then magnesium in the middle and zinc produced the least amount of hydrogen gas. This shows that the same mass of each metal does not produce the same amount of hydrogen gas. Looking at the balanced equations for each of the metals (see lab 2-1, equation 1 and 2), it seems the metals have a similar stoichiometry, however zinc produced a lesser amount of hydrogen gas compared to magnesium because zinc has a higher molar mass than magnesium does. Due to this, more zinc is needed to produce the same amount of hydrogen gas as magnesium. When aluminum and magnesium are compared, it is seen that aluminum and magnesium have similar molar masses, however they have a different stoichiometry (experiment 2-1, equation 1 and 3). Two moles of aluminum react to produce three moles of hydrogen gas, while one mole of magnesium react to produce one mole of hydrogen gas. Based on this stoichiometry, a higher mass of magnesium is needed to produce the same amount of hydrogen gas as

In this project, C. Elegans are hermaphrodite worms that will be used since they are easy to maintain in lab, as well as have short life cycles. The gene that the project attempted to knockdown in C. Elegans with RNAi treatment is the unc-22 gene. RNAi disrupts gene expression in the presence of double stranded RNA (dsRNA) that is complementary to target gene sequence. The unc-22 gene codes for a muscle protein called twitchin in wild-type worms. The Unc-22 is required for muscle regulation and maintenance in C.Elegans. To verify that the RNAi treatment worked, would check the unc-22 mRNA levels in the worms, in addition to phenotype observation.

Today with my group lab we had to discuss on how to design an experiment that investigated the two herbicides DCMU and DCPIP. We used Elodea leaf and Elodea is basically a genus of aquatic plants often called the waterweeds and can be found anywhere in a pond or under water. So we started by creating a solution of phenol red, by adding 5 drops of concentrated phenol red to 40mL of water, then one of our group member used a straw to gently blow air into the solution until it reaches a neutral pH. We then transferred the solution into two test tubes evenly and labeled each tube dark and light, meaning the dark one will stay in the dark and the light one will stay under light bulbs. We predicted that dark one will stay the same and the light

2. (5 pts) List and explain the names and affiliations of the various characters/stakeholders in this story – I’m looking for us to use the story to map out the complexities that are generally associated with solving public health puzzles – the stakeholders you list and explain here should apply to many of the cases we consider going forward.

Therefore the more active element takes over, the equation changes, and a reaction takes place. The fourth reaction, zinc and hydrochloric acid, produced a gas, hydrogen gas. The final test was between copper and hydrochloric acid, which resulted in no reaction. Nothing occurred because the hydrogen is more active than the copper, thus the solution does not change. This lab was successful in showing the effect of a chemical reaction and how single replacement reactions

This is done through a change in temperature. Over time, two objects that are in direct contact will

2. When 2.00 g of NaOH were dissolved in 49.0 g water in a calorimeter at 24.0 ˚C, the temperature of the

However, with each solution, one metal was not mixed. When mixed with hydrochloric acid, students observed that Magnesium immediately started to bubble, emit gas, and fizz intensely. Fe and Zn bubbled too, however it was much more subtle. Cu appeared to have no initial reaction as it did not emit gas, it did not change color, and it did not fizz or bubble, all of which are signals a reaction is happening. This is because a fizzing or bubbling indicates gas is being released, in this case the gas was H2, and the change of color physically shows something is changing

The mean voltage of the battery terminals while connected to the identification resistors is presented in Figure ‎4 12. These samples have been pulled out from the voltage sensor of the PEB panel. The voltage decreased as expected from 12.53 to 12.5 during first 20 seconds of connection to the

3CuCl2 reacts with 2AlCl3 to create 2AlCl3 and 3Cu. CuCl was the limiting reactant in this lab. The CuCl can only make a specific amount of copper therefore, limits the amount produced and means Al is the excess reactant.

October 17, 18, and 19, samples were collected from multiple sites along the BSR. The class was split into groups, and samples were collected from seven separate locations along the river and WWTP. There was also a sample collected by the S which is located between sites four and five. For each of these sites, there were ten groups from other labs that also collected a sample from the BSR. At site two of the river, the location included multiple sources of possible contamination. A drainage site was located 200 yards upstream, along with a small PVC drainage pipe next to the collection site. Not only was there drainage running into the river, the site was under a bridge, and contained other trash scattered throughout the area. The

When mixed with hydrochloric acid (appendix 4), they react violently, hence why only a small portion was allowed for this experiment. This supports the hypothesis, that is, it was predicted that such a reaction would occur as these metals are highly reactive, hence why the hydrogen gas produced was clearly visible (appendix 5). Tin is less reactive, however, according to the Metal Reactivity Series, reacts with acids at an extremely slow rate. This was evident in the experiment; however, more of a reaction would have occurred if the time frame was expanded. The metal was only left in the acid for five minutes; therefore, it had no reaction but could of, had it been left a while longer. Magnesium and Calcium are both alkaline earth metals which means that they all have an oxidation number of ‘+2’, making them highly reactive. Calcium is more reactive than Magnesium even though it is located below it on the periodic table (appendix 6) because its electron configuration is ‘2,8,8,2’ while Magnesium’s is ‘2,8,2’. This means that Calcium has more shells which, therefore, means that there is less of an attraction to the nucleus. This makes it easier for Calcium to lose electrons and react more so than Magnesium. According to the Metal Reactivity Series, in order from the most reactive to the least reactive, tin is located at around the middle of the

The main purpose of this experiment was to show that single displacement reactions between metals according to their reactivity, with more reactive elements having the power to displace less reactive elements and take their place in a chemical compound (Beran, 2014). This was supported by the results of the experiment, where solid metals were combined with aqueous solutions that contained another element, and reactions only took place when the solid metal was more reactive than the other element in the compound. Only three attempted trials resulted in a failure to produce a reaction, namely the combinations of copper with hydrochloric acid, and copper with nickel sulfate. The outcomes of these trials are justifiably reasonable because copper is ranked lower in the