Chemical Reaction Lab

The Vitamin C turned to a red/orange color with no physical/chemical reaction. For the salt the solution turned to an orange color with no physical/chemical reaction. With the Alka-Seltzer, the solution turned to a brown color with no reaction as well. Last but not least, the Baking soda turned to an orange/brown color with no reaction.

Change in color once chemicals were combined (experiments b,c,d,e,f,g,h,j,l); Precipitate formation (experiments g,j,l), and formation of gas bubbles (experiment a).

: During each reaction, something happened. During reaction 1, after adding the nitric acid a red-brown gas was created. The copper first turned green after a few minutes turned into a blue solution. Reaction 2, When acid was added a blue precipitate formed. Reaction 3, when heated the solution turned into a black precipitate.

10 Solution Mystery Rehan Virani Chem 1212L-145 October 20, 2014 Purpose: The purpose of this experiment is to understand how Ksp values work. Also I will see how certain solutions react to other solutions.

Julene Thai 06/10/15 CHM 120-5 Sequencing copper chemical reactions Purpose: To see how much copper can be recovered after a series of chemical transformations. Pre-Laboratory Assignment: (a) It must be carried out under a fume hood because the oxidation of Cu with HNO3 solution produces NO2 gas, which is toxic. (b) One should be particularly careful when using concentrated HNO3 solution because it is highly toxic and an oxidant.

Materials We did several different examples of chemical equilibriums using different stresses and conditions. This includes adding or removing reactants, changing temperature, or adding additional compounds. Our materials included a large variety of chemicals and equipment used to conduct our labs.

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 initial adding of the H2SO4 resulted in the bubbling of the metals present. In the trials that included Magnesium, the Magnesium particles rose as the H2SO4 bubbled. The Magnesium changed from a dull gray color to a bright silver color after reacting with the H2SO4. Sample Calculations Calculations were needed in order to determine the averages for each part of the experiment. Example for Part 1: (sum of final temperatures)/3 =

Introduction: When a chemical change occurs, the composition of matter has changed (Myers 2003). Physical changes are changes in appearance but not the actual substance (Carolina Biological Supply Company 2012). A change in state is a physical change (Brown et. al 2015). The formation, breaking, or rearrangement of chemical bonds cause chemical changes (Carolina Biological Company 2012).

As you go down the periodic table you can clearly see that the reaction decreases and this can be because the metals don’t really react as they should, this can be because when they get into contact with any of the substances they don’t really have a chemical reaction to them, this can be because they don’t react as they should when placed in acid. Aluminium –Copper there wasn’t really a reaction and this is because these metals didn’t really have any acid base substance in them. The other thing is that From this you can see that potassium reacted with everything and every substance that it was mixed to clearly showed a major reaction, this can be because of where it is placed in the periodic table, the fact that this is the last one from group 1 means that it is a metal that reacts really quickly because of the ion bonds it has on its outer layers, lithium is found at the top of the group 1 metals and this one clearly shows that it doesn’t really react that quickly and this can be because it isn’t a strong metal like potassium, the other thing you can see from lithium is that on all of them you can see there was a slow reaction this can be because of the ion bonds it may have and because this is a small metal it may not be stronger like the others. So clearly from the group 1 metals

Anaija Hilliard Dr. Agapito Chemistry 10 February 13, 2018 Lab Report Introduction: In this activity, the group dealt with four metals and six chemicals. They observed the different chemical reactions each metal made with each chemical. In the end, the group ended up with 24 chemical reactions, each distinct to a certain metal and its chemical.

Silver nitrate and copper metal led to the formation of silver precipitate. We also observed a color change towards the bottom where the copper was located. These results support that the type of reaction was single- replacement. The second experiment with hydrochloric acid was an example of decomposition. We observed that the substance started to bubble and so a gas was produced.

The purpose of this lab was to analyze the reaction between various metals and ionic compounds to test if they follow the Activity Series of metals. For the most part, our hypothesis was that when metals and ionic compounds (sulphates) were combined, they will react according to the Activity Series of metals. In our experiment we hypothesized that when magnesium metal and copper sulphate combines, it will produce an aqueous solution of magnesium sulphate and copper metal. When zinc metal and iron sulphate are combined, an aqueous solution of zinc sulphate and iron metal is produced. When iron and tin chloride are combined, iron chloride and tin are formed. When tin is combined with copper sulphate, an aqueous solution of tin sulphate and copper

Discussion/Analysis 1. a) The physical properties that I examined in this experiment are state (at room temperature), colour, clarity, and crystal shape. b) The chemical properties that I examined in this experiment are reactivity in water and in acid. 2.

As only 2 balloons expanded in size, the results did not provide solid evidence to completely support the hypothesis of the practical. Having said that, the magnesium reaction time clarified its high metal reactivity as it expanded to its optimal circumference in the 30 seconds provided. Similarly, copper did not react at all as expected due to its low metal reactivity. However, between the maximum and minimum metals, in terms of reactivity, aluminium, zinc and iron showed no sign of expansion in the 30 second observational time limits. Nevertheless, the aluminium balloon expanded after approximately 40 minutes. As neither zinc nor iron reacted in this time span, it was confirmed that aluminium had the second highest metal reactivity, as anticipated from the hypothesis. After the first, second and last metals in the metal reactivity series were established, the remainder had to be observed for their chemical reactions to make a valid conclusion under the time constraint provided. From the observations between zinc and iron, it was perceived that zinc was more reactive due to which more bubbles and gas had formed in the test tube containing acid as opposed to iron where only occasional bubbles had developed. The metal reactivity series was confirmed from the balloon expansions and the chemical changes that occurred.