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Oduvanchick [21]
3 years ago
9

A chemistry student is given 3.00 L of a clear aqueous solution at 17.° C . He is told an unknown amount of a certain compound X

is dissolved in the solution. The student allows the solution to cool to 17.° C . The solution remains clear. He then evaporates all of the water under vacuum. A precipitate remains. The student washes, dries and weighs the precipitate. It weighs 0.15 kg . Using the above information can you calculate the solubility, X, in water at 17 degrees C
Chemistry
1 answer:
Ray Of Light [21]3 years ago
3 0

Answer:

Solubility of X in water at 17°C is > 0,05 kg/L

Explanation:

When the solution is at 17°C the solution remains clear. That means that every X molecule is dissolved in water. The student obtained 0,15 kg of X in 3,00L of water. That means that under this conditions the concentration is:

\frac{0,15 kg X}{3,00L} = <em>0,05kg/L</em>

The solubility is defined as the concentration of a saturated solution. A saturated solution is a solution in which the solute (X) is in the maximum possible concentration. That means that <em>solubility of X in water at 17°C is > 0,05 kg/L</em> because X was completely dissolved in water and there is not enough data to obtain the exact solubility.

You need to add more X, heat the solution and then, cool it at 17°C obtaining a precipitate. The concentration of X substracting the mass of X that precipitate is the solubility of X in water.

I hope it helps!

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A 1500 kg race car accelerates at a rate of about 9M /s2 as to how much force does the engine need to create for this to happen
IgorC [24]

Answer:

13500 N

Explanation:

According to newtons second law of motion

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7 0
2 years ago
Copper has a specific heat of 0.385 J/gºC.
Anna71 [15]

Answer:

The final temperature is 348.024°C.

Explanation:

Given data:

Specific heat of copper = 0.385 j/g.°C

Energy absorbed = 7.67 Kj (7.67×1000 = 7670 j)

Mass of copper = 62.0 g

Initial temperature T1 = 26.7°C

Final temperature T2 = ?

Solution:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = T2 - T1

Q = m.c. ΔT

7670 J = 62.0 g × 0.385  j/g °C ×( T2- 26.7 °C )

7670 J = 23.87 j.°C ×( T2- 26.7 °C )

7670 J / 23.87 j/°C = T2- 26.7 °C

T2- 26.7 °C = 321.324°C

T2 = 321.324°C + 26.7 °C

T2 = 348.024°C

The final temperature is 348.024°C.

6 0
3 years ago
Find the total number of atoms in a sample of cocaine hydrochloride, c17h22clno4, of mass 23.0 mg .
Nataliya [291]
From the periodic table:
mass of carbon = 12 grams
mass of hydrogen = 1 gram
mass of nitrogen = 14 grams
mass of oxygen = 16 grams
mass of chlorine = 35.5 grams
Therefore,
molar mass of <span>c17h22clno4 = 17(12) + 22(1) + 35.5 + 14 + 4(16) = 339.5 grams

number of moles = mass / molar mass
number of moles = (23*10^-3) / (339.5)
number of moles = 6.77 * 10^-5 moles

number of atoms = number of moles * Avogadro's number
number of atoms = 6.77*10^-5 * 6.022*10^-23
number of atoms = 4.079 * 10^-27 atoms</span>
3 0
4 years ago
The Answers plz and thx
garri49 [273]

Answer:

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Explanation:

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