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Nuetrik [128]
3 years ago
13

A strand of hair is approximately 50 μm thick. If the diameter of an atom is 1 × 10-10 m, how many atoms thick is a strand of ha

ir?
Chemistry
2 answers:
Kazeer [188]3 years ago
6 0

Thickness of strand hair = 50 μm

Diameter of an atom  = 1 \times 10^{-10} m

Now, with the help of conversion factors, convert thickness in micrometer into meter i.e. 1 micrometer = 10^{-6}m

So, thickness of strand hair =50 μm= 50 \times 10^{-6} m

Therefore,

number of atoms thick is a strand of hair =  50 \times 10^{-6}m\times \frac{1 atom}{1 \times 10^{-10}m}

= 50\times 10^{4}atoms

Hence, number of atoms is 50\times 10^{4}atomsthick is a strand of hair.


alexandr402 [8]3 years ago
6 0

Answer : The number of atoms thick in a strand of hair are 5\times 10^5\text{ atoms}

Explanation : Given,

Diameter of an atom = 1\times 10^{-10}m

Thickness of strand of hair = 50\mu m=50\times 10^10^{-6}m

conversion used : 1\mu m=10^{-6}m

Now we have to determine the number of atoms thick in a strand of hair.

\text{Number of atoms thick}=\frac{50\times 10^10^{-6}m}{1\times 10^{-10}m}=5\times 10^5\text{ atoms}

Therefore, the number of atoms thick in a strand of hair are 5\times 10^5\text{ atoms}

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The number of moles of gas lost is  0.0213 mol. It can be solved with the help of Ideal gas law.

<h3>What is Ideal law ?</h3>

According to this law, "the volume of a given amount of gas is directly proportional to the number on moles of gas, directly proportional to the temperature and inversely proportional to the pressure. i.e.

PV = nRT.

Where,

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  • R =  gas constant, 8.314 J*(mol-K)

Therefore, the number of moles is

n = PV / RT

State 1 :

  • T₁ = (25⁰ C = 25+273 = 298 K)
  • p₁ = 225 kPa = 225 x 10³ N/m²

State 2 :

  • T₂ = 10 C = 283 K
  • p₂ = 185 kPa = 185 x 10³ N/m²

The loss in moles of gas from state 1 to state 2 is

Δn = V/R (P₁/T₁ - P₂/T₂ )

V/R = (1.75 x 10⁻³ m³)/(8.314 (N-m)/(mol-K) = 2.1049 x 10⁻⁴ (mol-m²-K)/N

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Therefore,

Δn = (2.1049 x 10⁻⁴ (mol-m²-K)/N)*(755.0336 - 653.7102 N/(m²-K))

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<u>Answer:</u> The \Delta G for the reaction is 54.6 kJ/mol

<u>Explanation:</u>

For the given balanced chemical equation:

CO_2(g)+CCl_4(g)\rightleftharpoons 2COCl_2(g)

We are given:

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\Delta G^o_{rxn}=\sum [n\times \Delta G_f(product)]-\sum [n\times \Delta G_f(reactant)]

For the given equation:

\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(COCl_2)})]-[(1\times \Delta G^o_f_{(CO_2)})+(1\times \Delta G^o_f_{(CCl_4)})]

Putting values in above equation, we get:

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Conversion factor used = 1 kJ = 1000 J

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We are given:

p_{COCl_2}=0.760atm\\p_{CO_2}=0.140atm\\p_{CCl_4}=0.180atm

Putting values in above equation, we get:

K_p=\frac{(0.760)^2}{0.140\times 0.180}\\\\K_p=22.92

  • To calculate the Gibbs free energy of the reaction, we use the equation:

\Delta G=\Delta G^o+RT\ln K_p

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\Delta G = Gibbs' free energy of the reaction = ?

\Delta G^o = Standard gibbs' free energy change of the reaction = 46900 J

R = Gas constant = 8.314J/K mol

T = Temperature = 25^oC=[25+273]K=298K

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Putting values in above equation, we get:

\Delta G=46900J+(8.314J/K.mol\times 298K\times \ln(22.92))\\\\\Delta G=54659.78J/mol=54.6kJ/mol

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