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makkiz [27]
2 years ago
12

In chemistry class, you are given a density column with golden syrup, water, and oil. Your teacher gives you an unknown substanc

e. The unknown substance is a solid, and it has been determined that the density of the unknown is 7.50 g/cm3. If this unknown solid was placed into the density tube, which of these best describe the outcome?
A) It would float on top of the oil.
B) It would sink directly to the bottom.
C) It would rest between the oil and the water.
D) It would float between the oil and the golden syrup.
Chemistry
2 answers:
maksim [4K]2 years ago
6 0

Answer:

The correct answer is option B) It would sink directly to the bottom.

Explanation:

Hello!

Let's solve this!

Generally, solids have a higher density than liquids. In this case the densities are differentiated between the syrup, the oil and the water.

I think the solid would sink to the bottom.

After the explanation, we conclude that the correct answer is option B) It would sink directly to the bottom.

Alika [10]2 years ago
3 0
Maybe the bottom because I am pretty sure the oil would be on top so it couldn't be D. because it would originally go Oil , Water , Golden Syrup
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General properties of matter include all but which of the following.
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General properties of matrer include all but color. Mass, density and Volume are tbe intensive properties of matter.
4 0
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Read 2 more answers
A 0.82 kg piece of wood floats in water but is found to sink in alcohol (sg=0.79), in which it has an apparent mass of 0.059 kg
schepotkina [342]
Upthrust = loss in weight = 0.82 - 0.059 = 0.761 Kg
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8 0
3 years ago
What mass of this substance must evaporate to freeze 190 g of water initially at 17 ∘C? (The heat of fusion of water is 334 J/g;
Nikolay [14]

The question is incomplete, here is a complete question.

\Delta H_{vap} of CCl_2F_2 is 289 J/g.  What mass of this substance must evaporate in order to freeze 190 g of water initially at 17 degrees C? (heat of fusion of water is 334 J/g; specific heat of water is 4.18 J/g.K).  

Answer : The mass of this substance evaporate to freeze must be, 258.2 grams.

Solution :

First we have to calculate the total heat absorbed.

\text{Total heat absorbed}=[m\times c_{p,l}\times (T_{final}-T_{initial})]+m\times \Delta H_{fusion}

where,

m = mass of water = 190 g

c_{p,l} = specific heat of liquid water = 4.18J/g.K

\Delta H_{fusion} = enthalpy change for fusion of water = 334J/g

T_{final} = final temperature = 17^oC=273+17=290K

T_{initial} = initial temperature = 0^oC=273+0=273K

Now put all the given values in the above expression, we get:

\text{Total heat absorbed}=[190g\times 4.18J/g.K\times (290-273)K]+190g\times 334J/g

\text{Total heat absorbed}=76961.4J

Now we have to calculate the mass of substance.

As, 298 J of heat are absorbed by 1 g of CCl_2F_2

So, 76961.4 J of heat are absorbed by \frac{76961.4J}{298J}\times 1g=258.2g of CCl_2F_2

Therefore, the mass of this substance evaporate to freeze must be, 258.2 grams.

7 0
3 years ago
Stoichiometry. Are my answers right?
OverLord2011 [107]

Answer:

Congratulations. Mostly correct.

Step-by-step explanation:

Part I. Gold

Moles of Au = 35.12 2g × 1/196.97 = 0.1783 mol Au

Atoms of Au = 0.1783 × 6.022 × 10²³/1 = 1.074 × 10²³ atoms Au

Part II. Sucrose

           Molar mass = 342.30 g/mol

Moles of C₁₂H₂₂O₁₁ = 1.202 g × 1/342.30

Moles of C₁₂H₂₂O₁₁ = 0.003 512 mol C₁₂H₂₂O₁₁

Moles of C = 0.003 512 × 12/1 = 0.042 14 mol C

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Atoms of C = 0.042 14 × 6.022 × 10²³  = 2.538 × 10²² atoms C

Atoms of H = 0.077 25 × 6.022 × 10²³ = 4.652 × 10²² atoms H

Atoms of O = 0.038 63 × 6.022 × 10²³ = 2.326 × 10²² atoms O

<em>Minor Quibbles: </em>

You put the moles of sucrose in the molar mass slot.

You got the wrong exponents for the atoms of C, H, O.

You followed the rules for significant figures for gold, but not for sucrose.

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