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TEA [102]
2 years ago
5

Hydrodistillation explain ????​

Chemistry
1 answer:
777dan777 [17]2 years ago
4 0

Answer:

Explanation:

Hydrodistillation is a traditional method for the extraction of bioactive compounds from plants. In this method, plant materials are packed in a still compartment then water is added in sufficient amount and brought to a boil. ... The vapor mixture of water and oil is condensed by indirect cooling with water.

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What pressure will be exerted by 26g if CO2 at a temperature of 35C and a volume of 550ml?
STALIN [3.7K]

Answer:

P = 28.5 atm

Explanation:

PV = nRT => P = nRT/V

P = Pressure = ?

n = moles of sample = mass/molar mass = 26g/44g·mol⁻¹ = 0.619 mole CO₂

R = gas constant = 0.08206 L·atm/mol·K

T = temperature in Kelvin = (35 + 273)K = 308K

V = volume in Liters = 550 ml = 0.550 L

Pressure (P) = nRT/V

= (0.619 mole)(0.08206 L·atm/mol·K)(308K)/(0.550 L) = 28.5 atm

3 0
3 years ago
a chemist makes of silver perchlorate working solution by adding distilled water to of a stock solution of silver perchlorate in
Elodia [21]

The concentration of the chemist's working solution is 6.718 mol/L.

Given,

The volume of silver perchlorate solution (V₁) = 790 ml.

The volume of distilled water added to the silver perchlorate(V₂) = 290ml.

The concentration of a stock solution of silver perchlorate (C₂) = 18.3 mol/L.

We have to find the concentration of the chemist's working solution (C₁).

As we know,

V₁C₁ = V₂C₂

From the above formula, we get,

C₁ = V₂C₂/V₁

C₁ = 290 × 18.3/ 790

C₁ = 6.718 mol/L

The concentration of the working solution = 6.718 mol/L

Hence, the concentration of the chemist's working solution is 6.718 mol/L.

To learn more about the concentration or stock's solution, visit: brainly.com/question/14510306

#SPJ4

7 0
1 year ago
Salt water has a density of 1.183g/mL. A ball has a density of 0.0134 g/mL. Will the ball float or sink?
madreJ [45]
The ball will float as it’s density is less than the salt water.
8 0
3 years ago
Iron, a metal, has which of the following features?
Nastasia [14]

Answer: A sea of electrons

Explanation:

4 0
3 years ago
What is the MOLAR heat of combustion of methane(CH₄) if 64.00g of methane are burned to heat 75.0 ml of water from 25.00°C to 95
melamori03 [73]

Answer:

-5.51 kJ/mol

Explanation:

Step 1: Calculate the heat required to heat the water.

We use the following expression.

Q = c \times m \times \Delta T

where,

  • c: specific heat capacity
  • m: mass
  • ΔT: change in the temperature

The average density of water is 1 g/mL, so 75.0 mL ≅ 75.0 g.

Q = 4.184J/g.\°C \times 75.0g \times (95.00\°C - 25.00\°C) = 2.20 \times 10^{3} J = 2.20 kJ

Step 2: Calculate the heat released by the methane

According to the law of conservation of energy, the sum of the heat released by the combustion of methane (Qc) and the heat absorbed by the water (Qw) is zero

Qc + Qw = 0

Qc = -Qw = -22.0 kJ

Step 3: Calculate the molar heat of combustion of methane.

The molar mass of methane is 16.04 g/mol. We use this data to find the molar heat of combustion of methane, considering that 22.0 kJ are released by the combustion of 64.00 g of methane.

\frac{-22.0kJ}{64.00g} \times \frac{16.04g}{mol} = -5.51 kJ/mol

8 0
3 years ago
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