In this experiment, groups were given two different unidentified substances with the goal of being able to figure out what chemical each substance was. Unidentified substance “2” was proven to be Tin (II) Chloride and the Unidentified substance “4” turned out to be Sodium Chloride. The conclusion that substance “2” was Tin (II) chloride could be proven due to the fact that it reacted with Zinc and Sodium Hydroxide. When Tin (II) chloride reacted with Zinc, it began bubbling. This occurred because there was a single replacement reaction between Tin (II) Chloride and Zinc. Zinc is far more reactive than Tin (II) Chloride, making this a very likely conclusion. In the experiment, Tin (II) Chloride should have reacted with the Sodium Hydroxide because …show more content…
Sodium Chloride and Sodium Hydroxide do not produce a reaction with one another, as both of the reactants contain sodium. In a reaction, these two products will stay apart from each other. Moving on, Sodium Chloride Zinc will also produce no reaction. This is because Sodium Chloride and Zinc perform a single replacement reaction. Since Zinc is much less reactive than Sodium Chloride, therefore mixing the substances together will not give you a reaction. In order for a single replacement reaction to work, the lone element has to be more reactive, or higher on the reactivity series, than the element it would be replacing. Because a double replacement reaction occurs between Sodium Chloride and Nitric Acid, one again, there would be no reaction. Double replacements produce two brand new compounds, an aqueous solution, and a substance in a different state of matter. This is caused by two compounds trading cations or anions to create two new compounds. Because two soluble chemicals are incapable of reacting with one another, the “Solubility Chart” must be considered when dealing with double replacement reactions. Since there is not reaction between Sodium Chloride and Nitric acid, as well as the other two chemicals, the conclusion that Sodium Chloride is what Substance “4” consists of
Discussion 1. Zn0 (s)+ Cu2+S6+O42-(aq) →Cu0(s) + Zn2+S6+O42-(aq) Zn0(s) → Zn2+(aq) + 2e- Cu2+(aq) + 2e- → Cu0(s) Zn0(s) + Cu2+(aq) → Zn2+(aq) + Cu0(s) Oxidant (oxidizing agent) is the element which reduces in experiment.
This experiment investigated the properties of metals by seeing the reactivity of metals. The metals used in this experiment were lithium, sodium, potassium, magnesium, and calcium. What was the first chemical change observed in the lab? Explain.
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
This means that all of the elements in the same group have a main aspect in common, except for a few exceptions. These elements react with the same specific compounds. This was used to identify the order of the groups from left to right and to determine which elements go under which group. Some research was conducted to identify all the names of the groups ranging from element number one to element number 20. Once all group names were recorded, it was researched which groups react with which compounds that are given on the element cards.
As it dissolves, it reacts with the water to form nitric acid, which lowers the pH of the solution as it is
Discussion A chemical reaction did occur in every combination, however no signs were shown for combination d) between sodium chloride and potassium nitrate. Indications of a chemical reactions occurring between these two compounds were not present, as in the colour did not change, and gas, heat, light nor sound was produced. In addition, when sodium chloride and potassium nitrate combine they form sodium nitrate and potassium chloride. The products sodium nitrate and potassium chloride are both aqueous, therefore no precipitate was formed either.
Even the average human body is mostly made up of nonionic compounds. An ionic compound is a chemical compound that is made up of ions that are held together by ionic bonding, which are electrostatic forces. An example includes sodium fluoride, sodium chloride, sodium bromide, etc. Nonionic compounds are substances that are made up of atoms, held together by covalent bonds. In this experiment, the independent variable make up the test substances, and the dependent variable consists of the observation, melting point, and conductivity.
Balanced Chemical Equation: Cu(s) + 4HNO3(aq) —> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) Reaction 2: when sodium hydroxide (NaOH) is added to copper (II) nitrate (Cu(NO3)2), a double displacement reaction will occur. Copper and sodium will displace each other to create copper (II) hydroxide and sodium nitrate. Balanced Chemical Equation: Cu(NO3)2 (aq) + 2NaOH (aq) —> CuOH2 (s) + 2NaNO3 (aq) Reaction 3: When copper (II) hydroxide is heated, a decomposition reaction will occur. The reaction will decompose forming two compounds, Copper (II) oxide, and water. Balanced Chemical Equation: Cu(OH)2 (s) + Heat —> CuO (s)
The solutions are copper nitrate, silver nitrate, zinc nitrate, and magnesium nitrate. If the element is in the alkali earth metals such magnesium than it should be more reactive with the solutions than most groups and the metals in the transition metals should have some reaction to some solutions. Alkali earth metals are pretty reactive while transition metals are less reactive. Analysis:
The carbonate test and the sulfate test gave no reaction to the unknown metal. Whereas, the halide test gave an off-white/cream colour. This proved that the non-metal part of the compound was Bromide. Evaluate: One error in this test was the observation of the colour of the flame. This is human error because the colour of the flame depends on the persons point of view (subjective).
Thus being said, if my partner and I were to perform this lab for a second time, we can agree that to improve our experiment results we would focus more on the chemical reaction that included zinc and hydrochloric acid, for this is the chemical reaction that we were not able to collect proper data and configure our results for. If we were able to re conduct only this part of the lab, based on previous experience, we would allow more time for the hydrogen gas to collect in hopes that adding a catalyst ( in this case heat) would evoke a reaction thus ensuring a
Q22. Can you give an example of a chemical reaction? Sodium chloride Chlorine is a harmful green gas when it is on it’s on its own and sodium is a highly reactive metal. When they are mixed together they make table salt.
This indicated that unknown 5 had acetate, and since there was only one option for an acid with acetate ions, the identity of unknown 5 was
Sodium and chlorine ions come together to form sodium chloride, or NaCl. When metals react with non-metals, electrons are transferred from the metal atoms to the non-metal atoms, forming ions. The resulting compound is called an ionic compound. Consider reactions between metals and non-metals, for example: Sodium + chlorine → sodium chloride.
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.