In a system ABC, a ternary alloy with composition of 30 wt. % B and 30 wt. %C consistsat a particular temperature of three phases of equilibrium compositionsas follows: Liquid phase: 50 % A, 40 % B, 10 % Casolid solution: 85 % A, 10 % B, 5 % CB solid solution: 10 % A, 20 % B, 70 % Ca. Plot the composition of the alloy.b. Calculate the proportion by weight of liquid, a and B present in this alloy.c. For the same temperature, find the composition of the alloy which willconsist of equal proportion of a and ß phases of the compositions statedabove, but with no liquid phase.

a system ABC, a ternary alloy with composition of 30 Wt. % B and 30 Wt. C consists at a particular temperature of three phases of equilibrium compositions as follows: Liquid phase: 50 % A, 40 % B, 10 % C asolid solution: 85 % A, 10 % B, 5 % C B solid solution: 10 % A, 20 % B, 70 % C a. Plot the composition of the alloy.

a system ABC, a ternary alloy with composition of 30 Wt. % B and 30 Wt. C consists at a particular temperature of three phases of equilibrium compositions as follows: Liquid phase: 50 % A, 40 % B, 10 % C asolid solution: 85 % A, 10 % B, 5 % C B solid solution: 10 % A, 20 % B, 70 % C a. Plot the composition of the alloy.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

World production of chromite (FeCr₂O₄), the main ore ofchromium, was 1.5107metric tons in 2003. To isolate chro-mium, a mixture of chromite and sodium carbonate is heated inair to form sodium chromate, iron(III) oxide, and carbon diox-ide. The sodium chromate is dissolved in water, and this solutionis acidified with sulfuric acid to produce the less soluble sodiumdichromate. The sodium dichromate is filtered out and reduced with carbon to produce chromium(III) oxide, sodium carbonate,and carbon monoxide. The chromium(III) oxide is then reduced to chromium with aluminum metal. (a) Write balanced equations for each step. (b) What mass of chromium (in kg) could be pre-pared from the 2003 world production of chromite?
Explain
4. From a pyrite concentrate containing 65% by weight pyrite (FeS,) by total oxdizer roasting, the following Fe,03 is produced according to the reaction. 5 tons of pyrite concentrate is reasted daily (MA, g/ mol; Fe 56; S: 32; O: 16; H: 1). 2FES2+11/20, Fe,03 + 450, If it is desired to produce 95% sulfuric acid from the flue gases, how much sulfuric acid by volume is produced in 1 day? (d.atunk anste 95%: 1.84 g/ cm2)
Blast furnace produces pig iron of composition Fe 94%, Si2%, Mn 0.5% and C 3.5% by reduction smelting of iron ore, coke and limestone. The analysis is as follows: Iron ore : Fe,0, 78%, SiO, 8%, Alz0, 5%, MnO 2% H20 7% Coke : 86% C and 10% S and 4% Al,0,; Amount is 600 Kg per ton of pig iron Limestone : pure Caco, to produce a slag of 45% Cao Calculate: a) Amount of ore/ton of pig iron b) % of total Si 0z and of Mn0 reduced in the furnace c) Amount of slag/ton of pig iron and its % composition.
A hypoeutectoid plain-carbon steel that was slow-cooled from the austenitic region to room temperature contains 9.1 wt% eutectoid ferrite. Assume that no change in structure on cooling from just below the eutectoid temperature to room temperature. Calculate the carbon content of the steel. Temperature ( 1000 900 7+ Fe,C 800 a+7 Eutectoid point 0.022 700 600 500- a+FqC 400 0 0.4 100% Fe 0.77 Pearlite Weight percent carbon Fe,C 6.67 1. Let x = the weight percent carbon of the hypoeutectoid steel (shown as a red line). Now, the relation (ratio) between the eutectoid ferrite to the total ferrite and the proeutectoid ferrite is expressed as: [Eutectoid Ferrite] = [Total Ferrite] - [Proeutectoid Ferrite) ... (eq.1) Fill eq.1 by using x. Express with up to 3 significant digits. (NOTE: Please check the rules for significant figures. For example, 0.012 and 1.23 both have 3 significant digits.) [Eutectoid Ferrite]-[1] [Total Ferrite]-[2] [Proeutectoid Ferrite]-[3] *Check the "Question Hint".…
a) A water source is to be treated using aluminium sulphate. The water has an alkalinity of 80 mg/l as CaCO3. Given the following information: Al2(SO4)3.14 H2O + 6HCO3- => 2Al(OH)3+ 6CO2 + 14H2O + 3SO4-2 Molecular weight of Al2(SO4)3.14 H2O = 594g Molecular weight of HCO3- = 61g Equivalent weight of HCO3- = 61g Equivalent weight of CaCO3 = 50g Determine the alkalinity remaining after the aluminium sulphate dose given in your datasheet has been applied. Comment on your answer.
A sample of steel weighing 2.00 g is analyzed for Cr (AW 52.0). The Cr is oxidized into chromate with alkaline permanganate and the excess permanganate is destroyed. A certain volume of 0.120 M FeSO4 is added to the acid solution and the excess is titrated with 0.0220 M KMnO4, requiring 31.0 mL. If the sample contained 0.50 % Cr, what volume (in mL) of FeSO4 was added?
Hand written please.
2. Calcium Flourite, CaF2, has a structure based on the fee lattice and a basis with Ca at and 333. Draw a projection diagram and sketch one 000 and F's at 1 conventional (cubic) cell of the structure.
If blast furnace slag is activated by NaOH, resulting in the formation of alkali-activated slag (AAS) – what kind of phases form in this system over time? How does the precipitated phase assemblage change with a change in the composition of the precursor slag? What differences exist in these formed phases in AAS systems when compared to blended systems such as OPC-Slag mixtures?
The assumptions about the virtual process state diagrams of metals A and B similar to the lead-tin system in Figure 9.8 are as follows. (1)The α phase and β phase exist at both ends of A and B. (2) The process composition is 36 wt% A to 64 wt% B. (3) The composition of β phase at the process temperature is 88 wt% A to 12 wt% B. Find the composition of an alloy in which the weight fraction of invitation β and total β is 0.367 and 0.768, respectively.
Calculate the saturation indices of the solutions described below and classify each as undersaturated, supersaturated, or in equilibrium. Saturation state with respect to: Anhydrite (CaSO4) [Ca2+] = 0.00002 mM [SO42-] = 25 mM “Amakinite” (Fe(OH)2) [Fe2+] = 0.1 mM; [OH-] = 0.0001 mM Siderite (FeCO3) [Fe2+] = 3 mM; [CO32-] = 10 mM