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kozerog [31]
3 years ago
12

1. The density of solid Cu is 8.96g/cm3 . How many atoms are present per cubic centimeter(cm3) of Cu ?

Chemistry
1 answer:
Leni [432]3 years ago
4 0

Answer:

8.5 × 10²² atom / cm³, 2.125 × 10²² unit cells / cm³, 4.7 × 10⁻²³ cm³ / cell unit, 3.61 × 10⁻⁸ cm /cell

Explanation:

The density of the solid Cu = 8.96 g/cm³

a) number of atoms present

mole = mass / molar mass = (8.96 g/cm³) / 63.546 = 0.141 mol

number of atoms = mole × avogadro's constant = 0.141 × 6.02 × 10²³ = 8.5 × 10²² atom / cm³

b) a face-centered cubic unit cell contains 4 atoms

8.5 × 10²² atom / cm³ / 4 = 2.125 × 10²² unit cells / cm³

c) the volume of a unit cell of the metal = reciprocal of  2.125 × 10²² unit cells / cm³  = 1 ÷ ( 2.125 × 10²² unit cells / cm³ ) = 4.7 × 10⁻²³ cm³ / cell unit

the edge length of a cell of cu = ∛(4.7 × 10⁻²³ cm³ / cell unit) = 3.61 × 10⁻⁸ cm /cell

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             %age Yield  =  51.45 %

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Step 1: Convert Kg into g

68.5 Kg CO  =  68500 g CO

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Step 2: Find out Limiting reactant;

The Balance Chemical Equation is as follow;

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According to Equation,

                   28 g (1 mol) CO reacts with  =  4 g (2 mol) of H₂

So,

                    68500 g CO will react with  =  X g of H₂

Solving for X,

                    X  =  (68500 g × 4 g) ÷ 28 g

                    X  =  9785 g of H₂

It shows 9785 g H₂ is required to react with 68500 g of CO but we are provided with 8600 g of H₂ which is less than required. Therefore, H₂ is provided in less amount hence, it is a Limiting reagent and will control the yield of products.

Step 3: Calculate Theoretical Yield

According to equation,

            4 g (2 mol) H₂ reacts to produce  =  32 g (1 mol) Methanol

So,

                          8600 g H₂ will produce  =  X g of CH₃OH

Solving for X,

                    X  =  (8600 g × 32 g) ÷ 4 g

                     X =  68800 g of CH₃OH

Step 4: Calculate %age Yield

                     %age Yield  =  Actual Yield ÷ Theoretical Yield × 100

Putting Values,

                     %age Yield  =  3.54 × 10⁴ g ÷ 68800 g × 100

                     %age Yield  =  51.45 %


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