When I mole of Fe2O3(s) reacts with H2(g) to form Fe(s) and H20(g) according to the following equation, 98.8 kJ of energy are absorbed. Fe,O3(s) + 3H2(g)- →2F¢(s) +3H20(g) Is this reaction endothermic or exothermic? What is the value of q? kJ

Table Q4 shows the solubility of liquid trichlorohexane in toluene (also liquid) at equilibrium at different temperatures, where species 1 is trichlorohexane and species 2 is toluene. These data are obtained at 1 atm. X1 0.037 0.050 0.085 0.135 0.199 0.288 0.364 0.482 0.500 0.585 Table Q4 Temperature (°C) 92.18 100.00 107.11 111.96 113.84 112.87 109.63 101.91 100.00 90.05 (a) Plot a properly labeled T-x₁ diagram of this binary mixture at 1 atm. (b) Estimate the composition of each phase at 110°C for this binary mixture. (c) At 110°C and 1 atm, trichlorohexane is added dropwise into an initially pure toluene until the mole fraction of trichlorohexane reaches 0.5. Assuming equilibrium is preserved during every addition of trichlorohexane, describe what you would see if the whole process is conducted in a transparent beaker. (d) At 100°C, determine the A12 and A21 in the two-constant Margules equation. Justify any assumptions that you make.

(a) Consider the following chemical reaction: 3FE203(s) + CO(g) → 2Fe304(s) + CO2(g) AH° = ? Use the following thermochemical data to determine the enthalpy change of this reaction. (6) 2FE2O3 (s) AH° = -1652 kJ 4Fe(s) + 302(g) C(s,graphite) + ½O2(g) → CO(g) 3Fe(s) + 202 (g) → CO2(g) AH° = -110.5 kJ Fe304(s) C(s,graphite) + O2(g) AH° = -1117 kJ AH° = +395.5 kJ (b) What is the standard enthalpy of formation of carbon dioxide? (2)

The equilibrium constant with respect to temperature can be expressed for the reaction: Cyclohexane (g)! <--> methylcyclopentane (g) as: LnK = 4.814-2059/T. If placed to react 3 moles cyclohexane in a 5 liter container at a certain temperature and when equilibrium is reached, 8000 J of heat is released, Calculate the temperature of the container.

Please help with the material balances!!!!! Please!!

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%…

One half-cell in a voltaic cell is constructed from a copper wire electrode in a 4.0 x 10-8 M solution of Cu(NO3)2. The other half-cell consists of a zinc electrode in a 0.75 M solution of Zn(NO3)2. Calculate the cell potential. You may need to use the following data: Zn²+ (aq) + 2 e¯ + Zn(s) E° = -0.763 V Cu²+ (aq) + 2 e → Cu(s) E° = +0.337 V Potential =

8.2 L of chlorine gas at 298 K and 3.0 atm is added to a rigid 4.0 L reaction vessel containing 3.2 moles of He gas and 2.4 moles of fluorine gas?  Chlorine and Fluorine gas react according to the following reaction at 298 K.                                                               Cl2 (g)    +    3 F2  (g)    à 2 ClF3 (g)               What is the partial pressure of ClF3 after the reaction is complete?                If the reaction proceeded with a percent yield of 40%, what would be the partial pressure of ClF3?

The reaction of carbon monoxide(g) with water(l) to form carbon dioxide(g) and hydrogen(g) proceeds as follows: CO(g) + H2O(l)  ---> CO2(g) + H2(g) When 10.2 grams of CO(g) react with sufficient H2O(l) , 1.02 kJ of energy are absorbed .What is the value of H for the chemical equation given?

For the following reaction, 20.4 grams of chlorine gas are allowed to react with 4.21 grams of water . chlorine(g) + water(1) hydrochloric acid(aq) + chloric acid (HCIO3)(aq) What is the maximum amount of hydrochloric acid that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams