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Leona [35]
2 years ago
6

A student predicts that a solution of ethanol (C2H5OH) and water will have a lower density at room temperature than that of pure

water. Which tools would most help the student test this prediction?
Will give brainly
Chemistry
2 answers:
ohaa [14]2 years ago
4 0

Answer:

It would probably be, something that can take up moisture to test it.

Explanation:

(to see if it can evaporate)

Lubov Fominskaja [6]2 years ago
3 0
It could probably be something that could take moisture to test it
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b-acting as a standard unit of measure

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Calculate the molarity of a solution of monoprotic KHP prepared by mixing a 0.5237 g KHP in 50.0 mL of water .
Sergio039 [100]

Answer:

M=0.0513M

Explanation:

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In this case, since the molarity of a solution is computed by dividing the moles of solute by the volume of solution, we notice we first need the moles of KHP as shown below:

n=0.5237g*\frac{1mol}{204.22 g} =0.00256mol

Next, the volume in liters:

V=50.0mL*\frac{1L}{1000mL}\\\\V=0.0500L

Thus, the molarity turns out to be:

M=\frac{n}{V}\\\\M=\frac{0.00256mol}{0.05000L} \\\\M=0.0513M

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3 0
3 years ago
Elements are organized into groups / families according to their physical and chemical properties. Identify the elements that's
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Answer:

1 valence - Alkali Metals: Li Lithium, Na Sodium, K Potassium

2 valence - Alkaline Earth Metals: Be Beryllium, Mg Magnesium, Ca Calcium

3 valence - Non-metals: B Boron, Al Aluminium

4 valence - Non-metals: C Carbon, Si Silicon

5 valence - Non-metals: N Nitrogen, P Phosphorus

6 valence - Non-metals: O Oxygen, S Sulfur, Se Selenium

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3 0
3 years ago
Calculate the energy required to heat 322.0g of ethanol from −2.2°C to 19.6°C . Assume the specific heat capacity of ethanol und
just olya [345]

Answer:

There is 17.1 kJ energy required

Explanation:

Step 1: Data given

Mass of ethanol = 322.0 grams

Initial temperature = -2.2 °C = 273.15 -2.2 = 270.95K

Final temperature = 19.6 °C = 273.15 + 19.6 = 292.75 K

Specific heat capacity = 2.44 J/g*K

Step 2: Calculate energy

Q = m*c*ΔT

⇒ m = the mass of ethanol= 322 grams

⇒ c = the specific heat capacity of ethanol = 2.44 J/g*K

⇒ ΔT = T2 - T1 = 292.75 - 270.95 = 21.8 K

Q = 322 * 2.44 * 21.8 = 17127.8 J = 17.1 kJ

There is 17.1 kJ energy required

3 0
3 years ago
A chemistry student needs 45.0mL of pentane for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the stud
Masja [62]

The mass of pentane the student should weigh out is

The density of pentane is 0.626 gcm-3

To calculate the mass of pentane following expression is used,

(Density is defined as the mass divide by volume)

Density = mass / volume

mass of pentane = Density of pentane * Volume of pentane

mass of pentane = 0.626 gcm-3 * 45.0 mL

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Here the unit of mass of pentane is g,

However the unit of density is gcm-3 and unit of volume is mL i.e. cm3

Hence,   Mass = gcm-3 * cm3

              Mass = g

The mass of pentane the student should weigh out is 28.17g

Learn more about Density on

brainly.com/question/1354972

#SPJ1

5 0
2 years ago
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