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
So, to determine the change in enthalpy we will employ Hess’s Law of heat summation: It states that the value of DH for a reaction is the same whether it occurs directly or as a series of steps (LeMay et al, 1996). We will perform the two following reactions: Mg + 2HCl ® MgCl2 + H2 and. MgO + 2HCl ® MgCl2 + H2O, determine their enthalpy changes (DHs), and they will then be “added” to that of a given equation, the combustion of water, H2 + 1/2 O2 ® H2O
The mass of Mg + the mass of O2=mass of MgxOx. Knowing the mass of
Does changing the length of the carbon chain effect the heat of combustion of water when heated for 2 minutes?
Text Box: CaCO3 + HCl = CaCl2 + CO2 + H2O calcium carbonate + hydrochloric acid = calcium chloride + carbon dioxide + water
CaCl2 + H2O + CO2
Investigating the Standard Enthalpy of Potassium Nitrate Stability --------- Stable. Strong oxidizer - contact with combustible material may cause fire.
Determination of the Enthalpy Change of a Reaction. Determine the enthalpy change of the thermal decomposition of calcium carbonate by an indirect method based on Hess' law. Determination of the Enthalpy Change of a Reaction. Determine the enthalpy change of the thermal decomposition of calcium carbonate by an indirect method based on Hess' law. Using the proposed method of obtaining results, these values were gathered.
The Enthalpy Change of Different Alcohols My aim is to compare the enthalpy change of combustion of different alcohols in relation to the structure of each molecule. The enthalpy change of combustion of a fuel is a measure of the energy transferred when one mole of the fuel burns completely. In a chemical reaction, bonds must either be made or broken, this involves an enthalpy change. The formation of bonds is exothermic, energy is lost to the surrounding; on the other hand, breaking bonds is endothermic, energy is taken in. I obtain the value for the enthalpy change of each fuel by using the formula: Energy transferred from the fuel=
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 aim is to find out if changing the concentration of the hydrochloric acid solution has an effect on the time taken for the reaction. The reaction that will take place is: Hydrochloric acid + Calcium Carbonate + Calcium Chloride + Water + Carbon dioxide 2HCl (aq) + CaCo3 (s) CaCL2 (aq) + H2O + CO2 (g). Collision theory - Collisions between reactant particles are needed. for the reaction to take place in order to form a product.
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
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
Fly ash reacts with calcium hydroxide when used as a partial replacement of OPC in the presence of water and in ambient temperature to form calcium silicate hydrate (C-S-H) gel during the hydration process of OPC. It has been found that fly ash can effectively replace OPC up to 60% by mass (Malhotra 2002; Malhotra and Mehta