13.43 Octane (C3H18) enters an engine and burns with air to give products with the dry molar analysis of CO2, 10.5%; CO, 5.8%; CH4, 0.9%; H2, 2.6%; 02, 0.3%; N2, 79.9%. Determine the equivalence ratio.
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- What is the water solubility of BaCO3 (Kep = 2.6 x 10-9) in a solution containing 0.40 M CO, (aq)? %3D1.5g sample contains sulfur S (aw332) has been dissolved. The sulfur is precipitated as BaSO4 (mw = 233). If the weight of the precipitate is 0.65g the * :percentage of sulfur in the sample is 5.95% 31.69% 7.82% 7.18% OThe hydrogen sulfide in a 75.0-g sample of crude petroleum was removed by distillation and uncollected in a solution of CdCl2. The precipitated CdS was then filtered, washed, and ignited to CdSO4. Calculate the percentage of H₂S in the sample if 0.115 g of CdSO4 was recovered.
- 1. A student synthesized 3.214g of Ni(NH3)„Cl2 from 4.023g of N¡C12•6H2O. He dissolved 0.81g of Ni(NH3)nCl2 in 40 mL of 1.0M HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 1T; H2O 18. (1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = ɛbc. (2) The student used 38.75 mL of 0.498M NaOH to neutralize excess HCl in 40mL of the sample. Calculate the mass percent of NH3 in the product.A sample of processed meat scrap weighing 4.000 g is digested with concentrated HSO. and Hg(catalyst) until the N present has been converted to NHHSO.. This is treated with excess NaOH, and the liberated NHs is caught in a 100-ml of H.SO. ( Iml 0.01860 g Na:OJ. The excess acid requires 57.60 ml of NaOH ( ImL = 0.12660 g potassium acid phthalate, KHCaH.OJ. Calculate the percentage protein in the meat scrap 4.(a) In 20 or less of yourown words define the term “leachate”and describe how it forms. (b) Previous records had shown that to prevent acute toxicity to organisms, the maximum mass of CdSO4 that should be allowed into the landfill was determined to be 0.1 kg. This was calculated using a standard concentration of Cd in mg/L where the volume of the leachate pond was used as 500 000L. (i) Provide the name of the CdSO4 compound. State the oxidation number of Cd in this compound (ii) You need to ensure that the concentration used to determine the mass of Cd allowed in the landfill, meets the current regulatory standard. Assuming that previous calculations determined that all of the CdSO4 would be deposited in the leachate pond, what standard concentration of Cd in mg/L was used to determine the maximum mass of allowable CdSO4?
- 2. An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HC. The resulting solution was diluted with water, and the iron(III) was precipitated as hydrous oxide Fe,03 .XH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe,03 (FW = 159.69). Calculate (a) the percent Fe (FW = 55.847) and (b) the percent Fe;04 (FW = 231.54) in the sample.6. The phosphorus content in a 0.3004-g sample was precipitated as (NH4);PO4 .12M0O3 a slightly soluble precipitate. The precipitate was filtered, washed, and further redissolved in acid. The resulting solution was treated with an excess of Pb²* resulting in the formation of 0.3017 g of PbMoO4. Calculate the % w/w of P2Os.||A 1.00 g sample of NaOH which has been exposed to the air for some time is dissolve in water and water and diluted to 500.0 ml. 100.0 ml of the solution is titrated with 0.1062 N HCl (MOH indicator) and requires 38.60 ml. A second 100 .0 ml portion is titrated with excess BaCl2, diluted to 250 .0 ml and filtered. 200.0 ml of this filtrate then require 29.62 ml of the HCl ( HpH indicator) . Calculate the % NaOH and Na2CO3 in the original sample.
- 15). If Ca(NO3) (aq) is slowly added to solution containing CO32– and SO42– what compound would precipitate out first given the solubility products (Ksp (CaSO4) = 2.4 x 10–5 and Ksp (CaCO3) = 8.7 x 10–9)? CaCO3 would precipitate first because it is least soluble. CaSO4 would precipitate first because it is least soluble. CaCO3 would precipitate first because it is more soluble. CaSO4 would precipitate first because it is more soluble.You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4. The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. In terms of Mg(OH)2 content, does the sample product conform to the USP requirement? Justify your answer through calculations.Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?