An FCC iron-carbon alloy initially containing 0.20 wt% C is carburized at an elevated temperature and in an atmosphere wherein the surface carbon concentration is maintained at 1.0 wt%. If after 48 h the concentration of carbon is 0.35 wt% at a position 3.9 mm below the surface, determine the temperature at which the treatment was carried out. You will need to use data in the two tables below to solve this problem.
Answers
Answer:
Hello the table required is missing attached below is the missing table
Answer : 1299.05 k
Explanation:
Given data :
concentration of carbon ( Cx ) at a position 3.9mm below surface = 0.35
concentration of carbon ( Co ) = 0.20
surface carbon ( Cs ) = 1
Determine the temperature at which the treatment was carried out
first we will determine the value of Z in the table attached
given that the value of erf ( Z ) for Z = 0.8125 from the table
= [tex]\frac{Z- 0.9}{0.95-0.9} = \frac{0.8125-0.797}{0.8209-0.797}[/tex]
make Z subject of the equation
Z = 0.932
next calculate the diffusion coefficient using the relation below
Z = [tex]\frac{x}{2\sqrt{Dt} }[/tex] ----- ( 1 ) where ; z = 0.932 , x = 3.9 mm , t = 48h
0.932 =
x = 3.9 mm = 0.0039 m
t = 48 h = ( 48 *60* 60 ) = 172800 secs
Insert values into equation 2
0.932 = [tex]\frac{0.0039}{2\sqrt{D * 172800} }[/tex]
[tex]\sqrt{D*172800}[/tex] = (0.0039 / 0.932 ) / 2
172800 * D =( 0.0021 )^2
therefore D = 2.55 * 10^-11 m^2/s
Finally calculate the temperature at which the treatment was carried out
D = [tex]Do exp(\frac{-Qd}{RT} )[/tex] ----- ( 3 )
D = 2.55 * 10^-11 m^2/s ,
Do = 2.3*10^-5 m^2/s ( gotten from Diffusion data table )
Qd = 148000 J/mol ( gotten from Diffusion data table )
R = 8.31 J/mol k ( gotten from Diffusion data table )
back to equation 3
D / Do = exp ( -17810 / T )
1.11 * 10^-6 = exp ( -17810 / T )
therefore T = -17810 / ln( 1.11 * 10^-6 )
= - 17810 / -13.71 = 1299.05 k
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A sample of 0.600 mol of a metal M reacts completely with excess fluorine to form 46.8 g of MF2.?
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Answer:
See Explanation
Explanation:
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a) There are 1.20 mol F in MF2.
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From the reaction equation;
M + F2 ----> MF2
Since the reaction is 1:1, 0.600 mol of MF2 is formed
Note that 1 mole of MF2 contains two moles of F and one mole of M
Hence, number of moles of F in MF2 = 2 * 0.600 mol = 1.20 mol F
Since 1 mole of M is contained in MF2, there are 0.600 moles of M in MF2.
If 1 mol of M forms 1 mole of MF2
And, 0.600 mol of M form 0.600 mol of MF2
Number of moles of MF2 = mass/molar mass
Number of moles of MF2 = 0.600 mol
Mass of MF2 formed = 46.8 g
Molar mass of MF2 = mass/Number of moles of MF2
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Answers
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Explanation:
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Answers
Answer:
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Answers
Answer:
See explanation
Explanation:
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The answer is (a)
.
.
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#KEEPONLEARNING
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Answers
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[ pls mark me brainliest i need one more to rank up tysm if u do ]
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Answers
Answer:
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Nose jajajajajaj si mr ayudas te ayudo