12.00 g of a potassium hydroxide, KOH solution is mixed with 40.00 g of lead (II) nitrate, Pb(NO3)2 solution. A clear solution of potassium nitrate, KNO3 and a white precipitate of lead (II) hydroxide, Pb(OH)2 are formed as products. If the actual reaction yields only 21.5 g of solid precipitate, determine the percentage yield.

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Aluminum sulfate can be made by reacting crushed bauxite ore with sulfuric acid, according to the following equation: Al2O3 + H2SO4 = Al2(SO4)3 + H2O The bauxite ore contains 55.4% by weight of aluminium oxide, the remainder being impurities. The sulfuric acid solution contains 77.7% pure sulfuric acid, the remainder being water. To produce crude aluminium sulfate containing 1798 lb of pure aluminium sulfate, 1080 lb of bauxite ore and 2510 lb of sulfuric acid solution are needed. a) Identify the excess reactant and limiting reactant.b) What percentage of the excess reactant was consumed?c) What was the degree of completion of the reaction?d) Illustrate the Law of Conservation of Mass.

Alumina from bauxite separation stage calculations A crucial step in the production of aluminum from bauxite ore is the separation of alumina from the remaining mineral impurities in the ore. In the Bayer process this is accomplished by treating bauxite with aqueous NaOH to produce NaAIO2 (alumina). NaOH(aq) + Al(OH)3(s) → NaAIO2(aq) + 2H2O(1) Since NaAIO2 is water soluble while the residual mineral constituents of bauxite are not, a separation can be achieved by allowing the minerals to settle out and decanting the aqueous solution of NAAIO2 and unreacted NaOH. In order to further recover any NAAIO2 entrained in the settled mineral solids, this "mud" is repeatedly washed with water and allowed to settle, and the wash water is decanted. The figure below shows one stage of this washing-settling process. Wash water Slurry - Open to air Mixer/Wash tank Setling tank Decanted solution System boundary Washed mud In this stage, a feed slurry consisting of 10 wt% solids, 11 wt% NaOH, 16 wt%…

• Iron metal can be produced by reducing iron(III) oxide with hydrogen: Fe,0;(s) + 3 H,(g) 2 Fe(s) + 3 H,0(g) = +141.5 J/K AH = +98.8 kJ; AS %3D (a) Is this reaction spontaneous under standard-state conditions at 25 °C? • (b) At what temperature will the reaction become spontaneous?

1. Ethanol forms a nearly ideal solution with iso-butanol. The vapour-liquid equilibrium data is given below in terms of the more volatile component (ethanol).A heated feed containing 60mole % ethanol enters a flash drum at a rate of 50 kmol/h and equilibrium separation is achieved. What fraction of the feed to be vaporized to have a bottom product containing not more than 50% ethanol. 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1 y* 0.196429 0.354839 0.485294 0.594595 0.6875 0.767442 0.836957 0.897959 0.951923 1

11.7 mole dichloromethane (CH2Cl2) enter a reactor with 21.6 mole hydrogen (H2) and 37.5 mole oxygen (O2).  The following reaction takes place: CH2Cl2 + H2 + 3/2 O2 → COCl2 + 2 H2O 6.4 mole of H2O are produced.  Calculate the extent of the reaction.

Ammonia can react with oxygen according to the following two reactions: 4 NH3 + 5 O2  →   4 NO + 6 H2O 2 NH3 + 3/2 O2 →  N2 + 3 H2O 28.3 mole NH3 enter the reactor, along with 165 mole O2.  The reaction proceeds to 0.62 fractional conversion of ammonia and the selectivity of NO over N2 is 3.6.  Determine the total mole exiting the reactor

Using the phase diagram here, at what temperature will a solution of 36 mole % A begin to boil? Temperature-Composition Phase Diagram for Compositions of Compounds A and B 500 450 400 350 300 250 200 150 100 50 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 Composition (mole fraction B) Temperature (°C)

The composition of a gas on a dry basis is 70.0 mol% N2,70.0 mol% N2, 13.0% O2,13.0% O2, 12.0% CO2,12.0% CO2, and 5.0% CO.5.0% CO. If the mole fraction of water is 0.110,0.110, what is the gas composition on a wet basis ?