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Bond [772]
3 years ago
13

So my science teacher says if you put water in a cup and then put oil in it the oil is "more dense than water" witch means the o

il will go to the bottom but I thought it would go to the top plz help so I can pass my quiz
Chemistry
2 answers:
Neporo4naja [7]3 years ago
7 0
The oil is heavier (aka "denser") than the water. It is more heavily packed with molecules than the water. The oil slowly seeps to the bottom and the water rises above it. The two do not immediately mix due to the insolubility of oil. I hope this helps and please don't forget to make me the Brainliest :-)
laila [671]3 years ago
6 0
The oil would sink, due to the density of it
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6) Determine la concentración de una solución que ha sido preparada añadiendo 80cc de agua a 320cc de solución alcohólica al 20%
Xelga [282]

Answer:

16% v/v es la nueva concentración de alcohol en la solución

Explanation:

El porcentaje volumen/volumen (% v/v) es definido como 100 veces la relación entre el volumen de soluto (Alcohol en este caso) y el volumen total de la solución (Agua + Alcohol). Para resolver esta pregunta necesitamos hallar el volumen de alcohol y el de agua:

<em>Volumen alcohol:</em>

320cc * (20cc etanol / 100cc) = 64cc etanol

<em>Volumen agua:</em>

80cc + (320cc-64cc) = 336cc agua

<em>% v/v:</em>

64cc / (336cc + 64cc) * 100

= 16% v/v es la nueva concentración de alcohol en la solución

3 0
3 years ago
How many grams of Cl2 are in 1.20 x 1024 Cl atoms?
Vaselesa [24]
<h3>Answer:</h3>

70.906 g

<h3>Explanation:</h3>

We are given;

  • Atoms of Chlorine = 1.2 × 10^24 atoms

We are required to calculate the mass of Chlorine

  • We know that 1 mole of an element contains atoms equivalent to the Avogadro's number, 6.022 × 10^23.
  • That is , 1 mole of an element = 6.022 × 10^23 atoms
  • Therefore; 1 mole of Chlorine = 6.022 × 10^23 atoms

But since Chlorine gas is a molecule;

  • 1 mole of Chlorine gas = 2 × 6.022 × 10^23 atoms

But, molar mass of Chlorine gas = 70.906 g/mol

Then;

70.906 g Of chlorine gas = 2 × 6.022 × 10^23 atoms

                                          = 1.20 × 10^24 atoms

Thus;

For 1.2 × 10^24 atoms ;

= ( 70.906 g/mol × 1.2 × 10^24 atoms ) ÷ (1.20 × 10^24 atoms)

<h3>=  70.906 g </h3>

Therefore, 1.20 × 10^24 atoms of chlorine contains a mass of 70.906 g

=  

5 0
3 years ago
Plz help with this it is the digestive system
Strike441 [17]

Answer:

see explanation for answer

Explanation:

salivary gland:  1

stomach: 2

small intestine: 6

liver: 4

gallbladder: 5

large intestine: 3

The answers correspond with the numbers on the text boxes, so you would drag number 1 to the salivary gland and so on.

5 0
3 years ago
Read 2 more answers
1.For the reaction P4 O10(s) + 6H2O(l) → 4H3PO4(aq), what mass of P
Alex17521 [72]
P₄O₁₀ + 6H₂O → 4H₃PO₄
The equation shows us that the molar ratio of
P₄O₁₀ : 6H₂O = 1:6

We also know that one mole of a substance contains 6.02 x 10²³ particles. We can use this to calculate the moles of water.
moles(H₂O) = (5.51 x 10²³) / (6.02 x 10²³)
= 0.92 mole
That means moles of P₄O₁₀ = 0.92 / 6
= 0.15

Each mole of P₄O₁₀ contains 4 moles of P. 
moles(P) = 4 x 0.15 = 0.6 mol
Mr of P = 207 grams per mol
Mass of P = 207 x 0.6
= 124.2 grams
5 0
3 years ago
Read 2 more answers
Calculate the molality of isoborneol in the product if, a) the melting point of pure camphor is 179°C and the melting point take
tresset_1 [31]

Answer:

The molality of isoborneol in camphor is 0.53 mol/kg.

Explanation:

Melting point of pure camphor= T =179°C

Melting point of sample = T_f = 165°C

Depression in freezing point = \Delta T_f=?

\Delta T_f=T- T_f=179^oC-165^oC=14^oC

Depression in freezing point  is also given by formula:

\Delta T_f=i\times K_f\times m

K_f = The freezing point depression constant

m = molality of the sample

i = van't Hoff factor

We have: K_f = 40°C kg/mol

i = 1 (  organic compounds)

\Delta T_f=14^oC

14^oC=1\times 40^oC kg/mol\times m

m=\frac{14^oC}{1\times 40^oC kg/mol}=0.35 mol/kg

The molality of isoborneol in camphor is 0.53 mol/kg.

8 0
3 years ago
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