Which of the following equations is correct? Oa. O a. AG = Ginitial – Gfinal %3D Ob. . 1G = AH - TAS %3D O G=S- PV Od G = H – PV O e. AG = AS – TAH
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- A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here and the I2 released is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the weight percent by volume of NaOCl in the sample. (Ma(NaOC:74,4 g/mol)To prepare a very dilute solution of K2Cr2O7 (294.18 g/mol), 0.661 g of K2Cr2O7 was transferred to a 250.0-mL volumetric flask and adding water to the mark. A sample of this solution of volume 1.000 mL was then transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Subsequently, 10.0 mL of the diluted solution was transferred to a 250.0-mL flask and diluted to the mark with water. What is the final concentration of K2Cr2O7 in this last solution?
- Calculate the limiting and excess reagent of 3I2 + 6KOH → 5KI + KIO3 + 3H2O with solutions. 950g=I2, 1500g=KOHAn ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)Use the following atomic masses (in g/mol):Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H = 1; N = 14.01; S = 32.06; Cl = 35.45; 2.) Limestone consists chiefly of mineral calcite (CaCO3). The carbonate content of 0.5413g of powdered limestone was measured by suspending the powder in water, adding 10mL of 1.392M HCl and heating to dissolve the solid and expel CO2. The excess acid required 39.96mL of 0.1004M NaOH for complete titration to a phenolphthalein end point. Find the % wt of calcite in limestone.
- Subject :- Chemistry How many grams of EDTA (336.21g/mol) are contained in 1mL of a 2000microM solution?A 19.51 ݃ sample of impure methylamine, which contains 72.58% (by mass) of CH3NH2 , isreacted with 30.81 ݃ of pure oxygen gas:4CHଷNHଶ(g) + 9Oଶ(g) ⟶ 4COଶ(g) + 10HଶO(ℓ) + 2Nଶ(g) In another experiment, this impure methylamine was used as follows: An unknown mass of the impure compound is dissolved in enough water to make 500.0 ݉ܮof solution. 20 ݉ܮ of this solution was transferred by pipette to a clean 250 mL volumetric flask andmade up to the mark. The molarity of the CH3NH2 in the final solution was determined to be 0.103 M.Determine the mass of CH3NH2 present in the original amount of impure compound used tomake this solution.One method of removing CO2(g) from a spacecraft is to allow the CO2 to react with LiOH. 2LiOH(s)+CO2(g)→Li2CO3(s)+H2O(l) How many liters of CO2(g) at 23.6 ∘C and 1.00 barr can be removed per 9 kg of LiOH consumed?
- Calculate the weight of pure sodium carbonate that is necessary to prepare 2.806 L of 0.223 N Na2CO3 (105.99 g/mol) from the primary-standard solid. Assume the solution is to be used for titrations in which the reaction is: CO32- + 2H+ ----> H2O + CO2 Express you answers in 3 decimal places500g of Al2S3 dissolved in H2O to make 15.0 L of solution. What is its normality?(MW: Al = 27g / mol S = 32g / mol H=1g/mol, O=16g/mol)A. 0.11 NB. 0.07 NC. 0.22 ND. 0.04 N The concentration of a 1500mL aqueous KCI solution was increased from 25.0 M to 80.0 M by evaporation. How much H₂O was removed? (MW: K= 39g/mol, Cl = 35g/mol, H = 1g / mol 0=16g/mol)A. 1.03 LB. 0.47 LC. 1968.75 mLD. 4.68.75 ml. Suppose that 15M of NaCl solution with a volume of 15L is heated and loses 2000ml of its water content. What would be the final concentration of your NaCl sample? (MW: Na = 23g / mol , Cl = 35q / mol, H=1g/mol,O=16g/mol)A. 3.75 MB. 0.0375 MC. 37.5 MD. 375.0 MConcentrated sulfuric acid has a density of 1.84 g/cm3 and is 95.0% by mass H2SO4. (Hint: assume a basis of 1.00 L of solution) a) What is the mass fraction of sulfuric acid in the solution? b) What is the molarity of this acid?
