The Enthalpy Values for the Reaction Between Calcium Carbonate and Calcium Oxide with Hydrogen Chloride [IMAGE] H3 [IMAGE]CaCO3 (s) CaO (s) + CO2 [IMAGE] [IMAGE] H1 HCl H2 HCl CaCl2 (aq) Results ======= Variables of CaCO3 ================== Mass of CaCO3 + weighing bottle 3.302 g Mass of empty weighing bottle 0.831 g Mass of CaC03 used 2.471 g Temperature of acid initially 18 C Temperature of solution after mixing 21 C Temperature change during reaction 3 C Variables of Temperature Mass of CaO + weighing bottle 2.362 g Mass of empty weighing bottle 0.936 g Mass of CaO used 1.426 g Temperature of acid initially 17 C Temperature of solution after mixing 27 C Temperature change during reaction 10 C Calculations ------------ v Heat Capacity x Temperature Change x Volume 1000 v Mass of Reactant Moles Ar v [IMAGE] H1 for the reaction between CaCO3 + HCl 4.2 x 3 x 50 630_ 0.63 1000 1000 2.471 0.025 Ca ® 40 x 1 = 40
2-ethyl-1,3-hexanediol. The molecular weight of this compound is 146.2g/mol. It is converted into 2-ethyl-1-hydroxyhexan-3-one. This compounds molecular weight is 144.2g/mol. This gives a theoretical yield of .63 grams. My actual yield was .42 grams. Therefore, my percent yield was 67%. This was one of my highest yields yet. I felt that this was a good yield because part of this experiment is an equilibrium reaction. Hypochlorite must be used in excess to push the reaction to the right. Also, there were better ways to do this experiment where higher yields could have been produced. For example PCC could have been used. However, because of its toxic properties, its use is restricted. The purpose of this experiment was to determine which of the 3 compounds was formed from the starting material. The third compound was the oxidation of both alcohols. This could not have been my product because of the results of my IR. I had a broad large absorption is the range of 3200 to 3500 wavenumbers. This indicates the presence of an alcohol. If my compound had been fully oxidized then there would be no such alcohol present. Also, because of my IR, I know that my compound was one of the other 2 compounds because of the strong sharp absorption at 1705 wavenumbers. This indicates the presence of a carbonyl. Also, my 2,4-DNP test was positive. Therefore I had to prove which of the two compounds my final product was. The first was the oxidation of the primary alcohol, forming an aldehyde and a secondary alcohol. This could not have been my product because the Tollen’s test. My test was negative indicating no such aldehyde. Also, the textbook states that aldehydes show 2 characteristic absorption’s in the range of 2720-2820 wavenumbers. No such absorption’s were present in my sample. Therefore my final product was the oxidation of the secondary alcohol. My final product had a primary alcohol and a secondary ketone
Then comparing the initial temperature of the water to the temperature after the reaction between various salts has occurred, I was able to determine which salt resulted in an exothermic reaction when combined with water. The NaCl and KNO3 were both endothermic reactions because the final temperature was less than the initial temperature. This means that heat was lost by the surroundings, the solution, and gained by the system, the reaction. MgSO4 was exothermic because its final temperature was greater than its initial temperature, which means that heat was gained by the solution and lost by the reaction. Therefore, MgSO4 was the best salt to use for the heat pack because it was the only salt we tested that released heat. After this, we ran three trials with varying volumes of water in order to find the volume ratio of salt to water that would produce a reaction that could release enough heat to raise the temperature of the solution by about 20°C. From this information, I could find the changes of enthalpy of the reaction, which was able to be a substitute for changes in heat content because the reaction took place at a constant
Text Box: CaCO3 + HCl = CaCl2 + CO2 + H2O calcium carbonate + hydrochloric acid = calcium chloride + carbon dioxide + water
The Effect of Temperature on The Rate Of Reaction Between Magnesium And Hydrochloric Acid Planning I'm planning on investigating how temperature effects the reaction between magnesium and hydrochloric acid, the experiment will show whether the reaction will speed up or slow down with the change in temperature. Temperatures will range from room temp up until 70 degrees. The investigation will be a fair test because all quantities will remain the same for each test, each test will use the same amounts of hydrochloric acid and same size of magnesium, also the concentration of the acid will also not be changed. APPERATUS; · Conical flask · Bunsen Burner · Thermometer · Tri-pod · Protective matt · Stopwatch · Gauze · Measuring jug · Goggles
Investigating the Standard Enthalpy of Potassium Nitrate Stability --------- Stable. Strong oxidizer - contact with combustible material may cause fire.
Investigating the Factors Influencing the Rate of Reaction Between Sodium Thiosulphate and Dilute Hydrochloric Acid
Investigating the Thermal Decomposition Of Metal Carbonates Aim: To investigate a range of metal carbonates and see if they thermally decompose. Thermal Decomposition INVESTIGATION [IMAGE] ------- Written By Tauqir Sharif ------------------------ Research: When a metal is thermally decomposed the bond between the metal and its carbonate (carbon and oxygen) is removed and the carbonate is released as carbon dioxide. Metal Carbonate = Metal Oxide + Carbon Dioxide Malachite is an ore of copper.
be yes as I will then be able to use enthalpy change of reaction to
Kinetic equations are utilized in this article to describe the dependence of the reaction between carbon and oxygen atoms and their environment. The research is trying to answer how the reaction area affects porous particles, especially carbon in this research article. Carbon combusts in two different modes, high-rate and low-rate. The high-rate combustion of the homogeneous reaction consumes the oxygen particles above the surface of the particle. The heterogeneous reaction inside the particle is endothermic, meaning that heat is absorbed thus decreasing the particle temperature resulting in a higher rate of combustion. The low-rate combustion does not allow the homogeneous reaction to happen, but instead only the heterogeneous reaction inside the particle, concluding that a higher temperature increases the rate of combustion.
The Effect of Temperature on the Rate of Reaction Between Sodium Thiosulphate and Hydrochloric Acid
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
the acid was at 14 C the magnesium took 141 seconds to react and 27 C
Rate of Reaction Between Calcium Carbonate and Hydrochloric Acid Plan: In my experiment I will measure the rate of reaction between calcium carbonate and hydrochloric acid. The rate of the reaction is the speed that the reaction takes place so by measuring the rate I will measure the amount of time the reaction takes. Hydrochloric acid is a strong acid that is found in digestive juices in the stomach, it is also used for cleaning metals before they are coated. Calcium carbonate has a few forms including chalk and limestone the main use of these two materials is in the making of concrete, which is used for many things such as buildings. When you put calcium carbonate and hydrochloric acid together they react to form calcium chloride, carbon dioxide and water.
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
Concrete is the widely used material for all infrastructural activities in the world. There is a huge demand for concrete usage nowadays next to water. Around the world, lot of attention have been paid in the last two decades to minimize environmental degradation caused by the concrete .Many studies have been carried out to develop alternative material for concrete in order to reduce its environmental impact. Concrete is produced conventionally by using Ordinary Portland Cement (OPC) as the primary binder. The production of Ordinary Portland Cement (OPC) causes many environmental issues. Due to the calcinations of limestone and fossil fuel combustion during the manufacture of ordinary Portland cement, carbon dioxide is released in the order