Give the product of the given reactants, balance the equation, and identify the type of changes the reaction is involved. C6H12O6 (aq) ----> ____________
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Give the product of the given reactants, balance the equation, and identify the type of changes the reaction is involved.
C6H12O6 (aq) ----> ____________
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- Give the product of the given reactants, balance the equation, and identify the type of changes the reaction is involved. CuO (s) + 2HCl (aq)----> ____________The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)Give the product of the given reactants, balance the equation, and identify the type of changes the reaction is involved. KI+ Br2----> ____________
- Toluene, C7H8 , is burned with 30% excess air. A bad burner causes 15% of the carbon to form soot (pure C) deposited on the walls of the furnace. What is the Orsat analysis of the gases leaving the furnaceA solution containing 0.402 49 g of CoCl2 ? xH2O (a solid with an unknown number of waters of hydration) was exhaustively electrolyzed to deposit 0.099 37 g of metallic cobalt on a platinum cathode by the reaction Co21 1 2e2¡Co1s2. Calculate the number of moles of water per mole of cobalt in thereagent. A good approach is to find moles of Co, moles of CoCl2, mass of CoCl2, and, by difference, mass of H2O in the sample.Vanadium(V) oxide reacts with calcium according to the chemicalequation below. When 20.0 moles of V20s are mixed with 20.0moles of Ca, which is the limiting reagent in the production of V(I)?V20s (s) + 5Ca(1) -> 2V(1) + 5CaO(s) a. CaOb. Vc. No reagent is limiting.d V205e. Ca
- 0.1724g of a mineral containing MnO₂ was dissolved and then treated with excess iodide according to the following unbalanced reaction: MnO2(s) + H+ → Mn²+ + I2 + H₂O The I₂ released was titrated with a solution of Na₂S2O3 0.07320 mol/L, requiring 14.65 mL to reach the point end of degree a) Determine the percentage of MnO₂ in the ore. b) When iodine solutions are used as titrants these are prepared by dissolving 1₂ in concentrated KI. Explain the reason for the need for KI in the preparation of these solutions?Among the products, which of the following is correct?An analyst was assigned to work a sample with minerals. This iron-containing sample was analyzed by dissolving a 1.3142g sample in concentrated HCl. The resulting solution was diluted with water and iron (III) was precipitated as the hydrated oxide Fe2O3 xH2O by the addition of HN3. After filtration and washing, the residue was calcined at high temperature to produce 0.5488g of pure Fe2O3 (159.69g / mol). Determine the following:a) the% Fe (55.847 g / mol) and the% Fe3O4 (231.54 g / mol) in the sample.
- A (3.6500 g) of impure ammonium aluminium sulfate (NH4Al(SO4)2)) was treated with ammonia (NH3(aq)) producing hydrous alumina Al2O3.xH2O. The collected precipitate was filtered, washed, and ignited at 1000 °C to give 0.4935 g Al2O3 (Mw 101.9635 g/mol). Determine: a. % Al2O3 b. %Al c. Express concentration of Al in ppm.The analysis of a product of combustion on dry basis, when C6H18 was burned with atmospheric air, is as follows: CO2=12%, CO=1.75%, O2=3.01%, N2=83.24%. Compute the actual air-fuel ratio.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.