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LenaWriter [7]
3 years ago
12

Calculate the mass of iron(III) oxide that contains a million iron atoms. Be sure your answer has a unit symbol if necessary, an

d round it to significant digits.
Chemistry
1 answer:
KiRa [710]3 years ago
8 0

<u>Answer:</u> The mass of iron (II) oxide that contains a million iron atoms is 2.6\times 10^{-17}g

<u>Explanation:</u>

We are given:

Number of iron atoms = A million = 1.0\times 10^6

The chemical formula of the given compound is Fe_2O_3

It is formed by the combination of 2 iron atoms and 3 oxygen atoms.

According to mole concept:

1 mole of a compound contains 6.022\times 10^{23} number of particles

1 mole of iron (II) oxide will contain = (2\times 6.022\times 10^{23})=1.2044\times 10^{24} number of iron atoms

We know that:

Molar mass of iron (II) oxide = 159.7 g/mol

Applying unitary method:

For 1.2044\times 10^{24} number of iron atoms, the mass of iron (II) oxide is 159.7 g

So, for 1.0\times 10^6 number of iron atoms, the mass of iron (II) oxide will be \frac{159.7}{1.2044\times 10^{24}}\times 1.0\times 10^6=2.6\times 10^{-17}g

Hence, the mass of iron (II) oxide that contains a million iron atoms is 2.6\times 10^{-17}g

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Volume= Mass/ Density= 20/184
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3 years ago
Consider the reaction below for which K = 78.2 atm-1. A(g) + B(g) ↔ C(g) Assume that 0.386 mol C(g) is placed in the cylinder re
borishaifa [10]

Answer:

1.65 L

Explanation:

The equation for the reaction is given as:

                        A            +            B           ⇄        C

where;

numbers of moles = 0.386 mol C  (g)

Volume =  7.29 L

Molar concentration of C = \frac{0.386}{7.29}

= 0.053 M

                        A            +            B           ⇄        C

Initial               0                           0                      0.530    

Change          +x                          +x                       - x

Equilibrium      x                           x                      (0.0530 - x)

K = \frac{[C]}{[A][B]}

where

K is given as ; 78.2 atm-1.

So, we have:

78.2=\frac{[0.0530-x]}{[x][x]}

78.2= \frac{(0.0530-x)}{(x^2)}

78.2x^2= 0.0530-x

78.2x^2+x-0.0530=0  

Using quadratic formula;

\frac{-b+/-\sqrt{b^2-4ac} }{2a}

where; a = 78.2 ; b = 1 ; c= - 0.0530

= \frac{-b+\sqrt{b^2-4ac} }{2a}   or \frac{-b-\sqrt{b^2-4ac} }{2a}

= \frac{-(1)+\sqrt{(1)^2-4(78.2)(-0.0530)} }{2(78.2)}  or \frac{-(1)-\sqrt{(1)^2-4(78.2)(-0.0530)} }{2(78.2)}

= 0.0204  or -0.0332

Going by the positive value; we have:

x = 0.0204

[A] = 0.0204

[B] = 0.0204

[C] = 0.0530 - x

     = 0.0530 - 0.0204

     = 0.0326

Total number of moles at equilibrium = 0.0204 +  0.0204 + 0.0326

= 0.0734

Finally, we can calculate the volume of the cylinder at equilibrium using the ideal gas; PV =nRT

if we make V the subject of the formula; we have:

V = \frac{nRT}{P}

where;

P (pressure) = 1 atm

n (number of moles) = 0.0734 mole

R (rate constant) = 0.0821 L-atm/mol-K

T = 273.15 K  (fixed constant temperature )

V (volume) = ???

V=\frac{(0.0734*0.0821*273.15)}{(1.00)}

V = 1.64604

V ≅ 1.65 L

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