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How can I determine with DRAWINGS or DIAGRAMS the composition of a phase, and the amount of the phases in a mixed phase region? Please, identify the starting alloy in terms of hypo eutectic or hyper-eutectic alloy. Show how to use the lever rule, so can I determine the composition of the phases and their relative amounts, in two different mixed-phase regions, for the same alloy.
Calculate the theoretical yield of C2H5Cl when 139 g of C2H6 reacts with 232 g of Cl2 , assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl .
calculate the pH of the resultant solution: (a) 0.00 mL, (b) 5.00 mL, (c) 25.00 mL, (d) 45.00 mL, (e) 50.00 mL, (f) 51.00 mL.
concentrated sulfuric acid used in the labortory is 95% by mass. calculate the mass of water in 100-g
If 3.0 ml of distilled water is added to 2.0 ml of 0.35 M CoCl2 solution , what is the concentration of the resulting solutions?
a 720-mL sample of water was cooled from 60 degrees celsius to 10 degrees celsius. How much heat was lost?
Which element will have five electrons in its Lewis symbol? a. argon b. boron
The equilibiurm constant Kc for the reaction below is 4,2 at 1650 degrees Celcius. H2(g)+CO2(g)---->H2O(g)+CO(g). Initially 0.80 mol H2 and 0.08 mol CO2 are injected into a 5.0-L flask
The equilibrium concentration of I2 is 0.0900M. What is the equilibrium constant, Kc , for the reaction at this temperature?
what is the underlying electronic reason for all periodic trends?
An aqueous solution is 22.0% by mass silver nitrate, AgNO3, and has a density of 1.22 g/mL. What is the molarity of silver nitrate in the solution?
Calculate the pH at the equivalence point for titrating 0.250 solutions of each of the following bases with 0.250 M HBr
The Ka of a monoprotic weak acid is 7.76 × 10-3. What is the percent ionization of a 0.127 M solution of this acid?
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