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Which is the balanced chemical equation for the synthesis of magnesium nitride from the elements magnesium and nitrogen?
Mg + N2 --> MgN2
3Mg + 2N -->Mg3N2
3Mg + N2 --> Mg3N2
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- Give typed full explanation A stock solution of lithium phosphate (Li3PO4, MM= 115.794361 g/mol) is prepared by dissolving 295.8 g Li3PO4 in deionized water to a final total volume of 1.000 L. Suppose a 1.000-mL aliquot is taken from this stock solution and transferred to a new container to which deionized water is added until the total volume is 50.00 mL. A new 1.000-mL aliquot is taken from this 50.00 mL solution and transferred to a third container to which deionized water is added until the total volume is 25.00 mL. Calculate the number of individual lithium ions (Li+) in the final 25.00-mL solution. Note that lithium phosphate is a strong electrolyte that completely dissociates in water (note that (aq) means the species is a solute in an aqueous solution): Li3PO4 (aq) 3 Li+ (aq) + PO43– (aq) Report your answer to two significant figures. Use scientific notation. Example: 1.0*10^23 (this notation means 1.0 1023)For the gravimetric determination of manganese, 1.8762 g of sample containing Mn was dissolved in acid solution and made up to 100 mL in a calibrated volumetric flask. A 25.00 mL aliquot of this solution was transferred to a beaker. The solution was heated to boiling and chemical substances required were added till precipitating MnNH4PO4. After filtering, rinsing, and igniting, 0.5365 g of Mn2P2O7 was obtained. Calculate the % manganese in the sample (Mn: 55, P: 31, O: 16 g/mol).Pyrolusite (MnO2) is dissolved in hydrochloric acid:MnO2 + HCl → MnCl2 + H2O + Cl2The chloride was passed into potassium iodide solution where it liberated iodine:Cl2 + KI → KCl + I2The iodine liberated was estimated by adding sodium thiosulfate, the reaction beingI2 + Na2S2O3 → NaI + Na2S4O6If 5.6 g of crystallized sodium thiosulfate, Na2S2O3 5H2O ,were used up, how many grams of manganese were present?MW (g/mole): I =126.9; Mn =54.94; Cl = 35.45; K = 39.09; Na = 23; S = 32
- A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.A risk is a source of potential damageChemical safety is a condition of being safe from the occurrence of chemical incidentsEnthalpy is shown in TCE'sTorrefaction is the process used in making a charcoalA.) If all 4 statements are trueB.) If 3 of the 4 statements are trueC.) If 2 of the 4 statements are trueD.) If only 1 of the 4 statements is trueE.) If none of the 4 statements is trueThe purity of hydrazine, N2H4 is determined by titration with iodine. A sample of the oily liquid weighing 1.4286 is dissolved in water and diluted to 1.00L in volumetric flask. A solution of 50.00mL aliquot is taken with a pipet and titrated with a standard iodine solution, requiring 42.41 mL. The iodine was standardized against 0.4123g of primary standard As2O3, by dissolving As2O3 in a small amount of NaOH solution, adjusting the pH to 8.0, and titrating, requiring 40.28 mL iodine solution. Calculate the percentage purity of the hydrazine.
- In the alloy containing sn pb and cd, the mole ratio sn/pb is 2.73/1 and the mass ratio of pb/cd is 1.78/1, the percentage of cd by mass in the alloyA. 1.4639 g sample of limestone was analyzed for Fe, Ca and Mg. The iron was determined as Fe2O3, yielding 0.0357 g Calcium was isolated as CaSO4, yileding a precipitate of 1.4058 g and Mg was isolated as 0. 0627 g of MgP2O7. Report the amount of Febas %w/w Fe2O3, Ca as %w/w CaO and Mg in the limestone sample as % w/w MgOGaseous F2reacts with water to form HF and O₂,. In NaOH solution, F₂, forms F⁻, water, and oxygen difluoride (OF₂,), ahighly toxic gas and powerful oxidizing agent. The OF₂, reacts with excess OH, forming O₂,, water, and F⁻. (a) For each reac-tion, write a balanced equation, give the oxidation state of O inall compounds, and identify the oxidizing and reducing agents.(b) Draw a Lewis structure for OF₂,, and predict its shape.
- A secondary step in the process to produce ultra-pure silicon forelectronic applications involves silicon tetrachloride with magnesium in a redox reaction:__SiCl + __Mg→ __Si + __MgClBalance the equation above and assign the oxidation numbers (O.N.) of the atoms in the reactants and products. REACTANTS SIDEO.N. of Si in SiCl : ______O.N. of Cl in SiCl : ______O.N. of Mg: ______PRODUCTS SIDEO.N. of Si: ______O.N. of Mg in MgCl : _______O.N. of Cl in MgCl : ______A sample of impure KI weighing 0.600 g is dissolved in water, the solution acidified, and 25.00 mL of 0.0400 M KIO3 (an excess ) is added. The iodate is reduced to I2 and the iodide is oxidized to I, The I2 is boiled off, the solution cooled, and an excess of pure KI is added to react with the unused KIO3. The I2 produced is titrated with 40.38 mL of 0.1053 N thiosulfate. Write the equations for the reactions which occurred and calculate the percentage of KI in the sample.Subject :- Chemistry How many grams of EDTA (336.21g/mol) are contained in 1mL of a 2000microM solution?
