(Co, Fe) doped (La, Ca) based chromites - (La0.8Ca0.2)(Cr0.9-xCo0.1Fex)O3
The transition metal doped perovskite compound, (La0.8Ca0.2) (Cr0.9-xCo0.1Fex) O3 (x=0.03, 0.06, 0.09, 0.12) was synthesized by mixing the powders of lanthanum oxide (La2O3, 99.99%), chromium oxide (Cr2O3, 99.99%), cobalt oxide (Co3O4, 99.99%), ferric oxide (Fe2O3, 99.99%) and calcium carbonate (CaCO¬3, 99.99%) in stoichiometric ratio according to the following equation.
0.4La2O3 + 0.2CaCO3 + ((0.9-x))/2Cr2O3 + 0.1/3Co3O4 + x/2Fe2O3 →
(La0.8Ca0.2)(Cr0.9-xCo0.1Fex)O3 +CO2 ↑ …… (1.2)
The appropriate quantities of starting materials were calculated by equation (1.2) and the molecular weights given in table 1.1. To synthesize (Co, Fe) doped (La, Ca) based chromites,
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Stoichiometric quantities of these powders were taken according to the following equation.
((1-x))/2 La2O3 + x CaCO3 + MnO2 → La1-xCaxMnO3 + CO2 ↑ …… (1.4)
Using the molecular weights of starting materials and by equation (1.4), the quantities of starting materials were calculated and given in table 1.5. These oxide powders were mixed and ground for 2 h using an agate mortar. These ground powders were then calcined in a tubular furnace at 1300 °C for 5 h for homogeneity. Then, the calcined powders were ground again using agate mortar for 3 h and further calcined at 1400 °C for 12 h. Thereafter, the powders were ground again by agate mortar for 3 h. These powders were then pelletized and the resultant pellets were further sintered at 1450°C for 15 h in a tubular furnace to get the required samples. The prepared
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Proper weight ratios of these oxide and carbonate powders were used according following equation.
( (1-x))/2 La2O3 + x SrCO3 + MnO2 → La1-xSrxMnO3 + CO2 ↑ …… (1.5)
The quantities of starting materials used are given in table 1.6. These weighed powders were mixed thoroughly and ground for 3 h using an agate mortar. Then, these ground powders were calcined at 1250 °C for 8 h. Then the calcined powders were ground again for 5 h using agate mortar and further sintered at 1400°C for 12 h. These sintered powders were ground once again for 3 h using agate mortar. The resultant powders were pressed into pellets and sintered at 1450 °C for 15 h. Then, the final sintered powders were ground again for further characterizations. The synthesized pellets of La1-xSrxMnO3, (x=0.3, 0.4 and 0.5) manganites are shown in figure
The mass of the compound was 0.806 grams. This means that there was a percent yield of 80.6%. Looking at the table it appears that the synthesized compound is Ca(NO3)2. The synthesized compound has the same color for the flame test, the same pH level, and the mean value from the conductivity test was extremely
This paper describes the methods used in the identification, investigation of properties, and synthesis of an unknown compound. The compound was identified as calcium nitrate by a variety of tests. When the compound was received, it was already known to be one of twelve possible ionic compounds. The flame test identified the presence of the calcium anion in the compound. The compound tested positive for the nitrate cation using the iron sulfate test. At this point it was hypothesized that the compound was calcium nitrate. Reactivity tests and quantitative analysis comparing the unknown compound with calcium nitrate supported this hypothesis. Synthesis reactions were then carried out and analyzed.
Heat crucible and lid to redness, cool it, and determine and record its mass to the nearest 0.01 g. 2. Place powdered hydrate in the crucible, but leave it slightly ajar. 3. Gently heat the covered crucible to avoid spattering. When there is no further tendency to spatter, strongly heat the crucible for about 5 minutes.
To start, two samples of 0.12501 grams and 1.2499 grams of the crystals was weighed out, using an analytical balance, and placed into two Erlenmeyer flasks. Each flask then received 60 mL of DI water, 6 mL of 6M H2SO4, and 1 mL H3PO4. Then, one flask was placed on a hotplate and heated to 80°C. While the solution was being heated, 120 mL of 6 molar potassium permanganate, KMnO4, was obtained and used to first rinse a burette and then fill the burette for titration procedures.
Purpose: Figuring out the physical and chemical properties of multiple known powders by completing a series of tests.
Purpose: To determine the percent magnesium by mass in magnesium oxide and to observe if the percentage composition is constant by comparing class results.
Also because of the carbonate test it was determined that there was a carbonate in the mineral. Results and Discussion The mass of the mineral before the roasting procedure was 0.507 grams. The mineral was weighed because it is needed to make the necessary calculations and to determine the mineral. The
The purpose of this lab was to test the law of definite proportions for the synthesis reaction of combusting magnesium. In this lab, the polished magnesium ribbon was placed in covered crucible and was heated in order for it to react with Oxygen presented in air and in water provided. The result showed that Magnesium oxide formed through chemical reaction was made up of 60.19% magnesium and 39.81% oxygen, which is approximate proportion of both particles in every Magnesium oxide compound. From this lab it can be concluded that the law of definite proportion stating that the elements in a pure compound combine in definite proportion to each other is factual.
The purpose of this experiment is to verify the formula of magnesium oxide based on the masses of magnesium and the product (MgO). We verify the formula firstly by calculating the empirical formula of magnesium oxide and then calculating creating the magnesium oxide itself- a magnesium ribbon is combined with oxygen in the presence of air through combustion and this forms MgO. The empirical formula of a compound is the simplest method of expressing a chemical formula in whole-number ratios of the constituent atoms that are consistent with masses measured in the experiment; whereas the molecular formula expresses the chemical formula using the actual number of atoms. For example, the molecular formula of anthracene is C14H10 while the empirical formula is C7H5.
Aim: To classify unknown substances according to their structure type and to observe how the structure of materials affects their uses.
1. Girolmi, G.S.; Rauchfuss, T.B.; Angelici, R.J. Synthesis and Technique in Inorganic Chemistry: A Laboratory Manual. University Science Books, 1999.
When the compound is crushed into a powder form it is used for making ceramics. (Lead(II)+chloride
In order to perform an artificial aging on these 4 samples, they are transferred into a 190°C Furnace, then are removed separately after 3, 10, 60, and 120 minutes; Then all quenched into water, and their hardness tested. In addition to the above process, the hardness test of the samples # 5 and 3 are measured after a week (table 4).
Purpose: To create chalk (calcium carbonate) and to find the percentage yield in order to see the amounts of anhydrous sodium carbonate and calcium chloride were used up. Also to see if there’s any alterations like mass differentials.