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3 years ago

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If you tested two samples of a particular pure substance, what would you find?

1 answer:

saw5 [17]3 years ago

3 0

Answer:

The properties of a pure substance can be used to determine whether a sample is a pure substance or mixture because the characteristic properties of matter can be used to identify a sample. The result is a mixture called a composite.

Explanation:

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Determination of the chemical composition of the atmospheres of the planets is carried out most effectively by what type of stud

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3 years ago

Lewis dot diagram for the Cs1+ ion

creativ13 [48]

Answer:

$Cs^+$

Explanation:

Cesium Lewis dot structure would look like this:

·Cs, because it only has one valence electron. But, since it has a plus, that means we lost an electron. So, we have to get rid of the dot and you have:

$Cs^+$

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2 years ago

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3 years ago

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If you added 15,000 calories to 2.0 L of water that was at 25.0 degrees C, what temperature would it be at when you finished?

rewona [7]

<u>Answer:</u>

<em>When we finish, the temperature would be 32.5℃</em>

<em></em>

<u>Explanation:</u>

Density of water = mass/volume

So,

Mass of water = Density × Volume

$\\\\$=1.0 \times 2.0 L$\\\\$=1.0 \frac{g}{m L} \times 2000 m L$\\\\$\quad=2000 g$$

$Q=m \times c \times \Delta T$

where

$\Delta T$ = Final T - Initial T

Q is the heat energy in calories

c is the specific heat capacity (for water 1.0 cal/(g℃))

m is the mass of water

plugging in the values

$15000 \mathrm{Cal}=2000 \mathrm{g} \times 1.0 \frac{\mathrm{cal}}{\mathrm{g}^{\circ} \mathrm{C}} \times \Delta T$

$\\$\Delta T=\frac{15000 \mathrm{cal}}{2000 \mathrm{g} \times \frac{1.0 \mathrm{cal}}{g^{\circ} \mathrm{C}}}$\\\\$\Delta T=7.5^{\circ} \mathrm{C}$$

Final T = ∆T + Initial T

= 7.5℃ + 25℃ = 32.5℃ (Answer).

5 0

2 years ago

How many grams of iron can be made with 21.5g of Fe2O3

SIZIF [17.4K]

The mass (in grams) of iron, Fe that can be made from 21.5 g of Fe₂O₃ is 15.04 g

We'll begin by writing the balanced equation for the reaction. This is given below:

2Fe₂O₃ -> 4Fe + 3O₂

Molar mass of Fe₂O₃ = 159.7 g/mol
Mass of Fe₂O₃ from the balanced equation = 2 × 159.7 = 319.4 g
Molar mass of Fe = 55.85 g/mol
Mass of Fe from the balanced equation = 4 × 55.85 = 223.4 g

From the balanced equation above,

319.4 g of Fe₂O₃ decomposed to produce 223.4 g of Fe

<h3>How to determine the mass of iron, Fe produced</h3>

From the balanced equation above,

319.4 g of Fe₂O₃ decomposed to produce 223.4 g of Fe

Therefore,

21.5 g of Fe₂O₃ will decompose to produce = (21.5 × 223.4) / 319.4 = 15.04 g of Fe

Thus, 15.04 g of Fe were produced.

Learn more about stoichiometry:

brainly.com/question/9526265

#SPJ1

5 0

1 year ago