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3 years ago

What is the working principle og fractional distillation?

Chemistry

1 answer:

Tanzania [10]3 years ago

7 0

Answer:

The basic principle of this type of distillation is that different liquids boil and evaporate at different temperatures. So when the mixture is heated, the substance with a lower boiling point starts to boil first and convert into vapors. Let consider a liquid-liquid mixture of A and B where A is more volatile than B this mixture can be separated by the following process:

Explanation

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If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what is the difference between the ideal pressure (as predict

yan [13]

Answer:

The answer to your question is:

Explanation:

Ideal gases

PV = nRT

P = nRT / V

P = (1)(0.082)(303) / 0.5

P = 49.7 atm

Real pressure

P = V²(nRT)/ (V - nb) - an²

P = (0.5)²(1)(0.082)(303) / (0.5 - (1)(0.03219) - (1.345)(1)²

P = (6.2115)/(0.4678) - 1.345

P = 13.28 - 1.345

P = 11.93 atm

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4 years ago

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pshichka [43]

Answer:

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3 years ago

3. During an experiment where 50.0 mL of a 1.0 M acid solution was mixed with 50.0 mL of a 1.0 M base solution, the temperature

Aleksandr-060686 [28]

Answer:

$\large \boxed{\text{-61 kJ$\cdot$mol$^{-1}$}}$

Explanation:

Data:

H₃O⁺ + OH⁻ ⟶ 2H₂O

V/mL: 50.0 50.0

c/mol·L⁻¹: 1.0 1.0

ΔT = 6.5 °C

ρ = 1.210 g/mL

C = 4.18 J·°C⁻¹g⁻¹

C_cal = 12.0 J·°C⁻¹

Calculations:

(a) Moles of acid

$\text{Moles of acid} = \text{0.0500 L} \times \dfrac{\text{1.0 mol}}{\text{1 L}} = \text{0.0500 mol}\\\\\text{Moles of base} = \text{0.0500 L} \times \dfrac{\text{1.0 mol}}{\text{1 L}} = \text{0.0500 mol}$

(b) Volume of solution

V = 50.0 mL + 50.0 mL = 100.0 mL

(c) Mass of solution

$\text{Mass of solution} = \text{100.0 mL} \times \dfrac{\text{1.10 g}}{\text{1 mL}} = \text{110.0 g}$

(d) Calorimetry

There are three energy flows in this reaction.

q₁ = heat from reaction

q₂ = heat to warm the water

q₃ = heat to warm the calorimeter

q₁ + q₂ + q₃ = 0

nΔH + mCΔT + C_calΔT = 0

0.0500ΔH + 1.10×4.18×6.5 + 12.0×6.5 = 0

0.0500ΔH + 2989 + 78.0 = 0

0.0500ΔH + 3067 = 0

0.0500ΔH = -3067

ΔH = -3067/0.0500

= -61 000 J/mol

= -61 kJ/mol

$\text{The enthalpy of reaction is $\large \boxed{\textbf{-61 kJ$\cdot$mol$^{\mathbf{-1}}$}}$}$

Note: The answer can have only two significant figures because that is all you gave for the change in temperature.

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3 years ago

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Furkat [3]

Answer:

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3 years ago

Calculate 18.9 minus 2.15. Round the answer to the correct number of significant figures.

Lerok [7]

The answer is 16.75 it rounds to 17 Hope this helps! ;D

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4 years ago

What is the working principle og fractional distillation?​

What is the working principle og fractional distillation?