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Lina20 [59]
3 years ago
12

An alloy contains 59g of pure silver and 19g of pure copper. What is the silver in the alloy

Chemistry
1 answer:
Lyrx [107]3 years ago
6 0

59+19=78

78----->59

100------>59*100/78

this percentage silver in the alloy

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Johannes Kepler, an apprentice of Brahe, believed in the heliocentric universe but rejected past astronomers' belief in
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<span>Johannes Kepler, an apprentice of Brahe, believed in the heliocentric universe but rejected past astronomers' belief in "Circular Orbit Path." The circular orbit path refers to the path the planets in the solar system is following. It is believed before that it follows a circular path rather than an elliptical one.</span>
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4 years ago
Which statement best describes how her tissue are responding to he running​
bija089 [108]

Answer:

When Kristen is running and her breathing rate increases, the statement that best describes how her tissues are responding to her running is that they need more oxygen to function, so gas exchange needs to increase.

Explanation:

Options for this question are:

They need more oxygen to function, so gas exchange needs to decrease.

They need more oxygen to function, so gas exchange needs to increase.

They need more carbon dioxide to function, so gas exchange needs to increase.

They need more carbon dioxide to function, so gas exchange needs to decrease.

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Explanation:

6 0
3 years ago
What color do you get if you mix red and blue light?
andrezito [222]

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5 0
3 years ago
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When of a certain molecular compound X are dissolved in of benzene , the freezing point of the solution is measured to be . Calc
puteri [66]

The question is incomplete. Here is the complete question.

When 2.10 g of a certain molecular compound X are dissolved in 65.0 g of benzene (C₆H₆), the freezing point of the solution is measured to be 3.5°C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.

Answer: MM = 47.30 g/mol.

Explanation: There is a relationship between <u>freezing</u> <u>point</u> <u>depression</u> and <u>molality</u>. With this last one, is possible to calculate <u>molar</u> <u>mass</u> or molar weight of a compound.

<u>Freezing</u> <u>Point</u> <u>Depression</u> occurs when a solute is added to a solvent: the freezing point of the solvent decreases when a non-volatile solute is incremented.

<u>Molality</u> or <u>molal</u> <u>concentration</u> is a quantity of solute dissolved in a certain mass, in kg, of solvent. Its symbol is m and it's defined as

m=\frac{moles(solute)}{kg(solvent)}

Freezing point depression and molal are related as the following:

\Delta T_{f}=K_{f}.m

where

\Delta T_{f} is freezing point depression of solution

K_{f} is molal freezing point depression constant

m is molality

Now, to determine molar mass, first, find molality of the mixture:

\Delta T_{f}=K_{f}.m

m=\frac{\Delta T_{f}}{K_{f}}

For benzene, constant is 5.12°C/molal. Then

m=\frac{3.5}{5.12}

m = 0.683 molal

Second, knowing the relationship between molal and moles of solute, determine the last one:

m=\frac{moles(solute)}{kg(solvent)}

mol(solute)=m.kg(solvent)

mol(solute) = 0.683(0.065)

mol(solute) = 0.044 mol

The definition for <u>Molar</u> <u>mass</u> is the mass in grams of 1 mol of substance:

n(moles)=\frac{m(g)}{MM(g/mol)}

MM=\frac{m}{n}

In the mixture, there are 0.044 moles of X, so its molecular mass is

MM=\frac{2.1}{0.044}

MM = 47.30 g/mol

The molecular compound X has molecular mass of 47.30 g/mol.

7 0
3 years ago
Write the symbol for nitrogen which has 9 neutrons<br><br>How do I solve this?
diamong [38]
If you mean lewis dot symbol you need a nuclide you get the number of proton (z) its equal to electrons since the atom is nutral then you make the elctron configuraion after that you take the number of electrons on the outer energy level( ex:k²L² in this case its the 2 on the L)and if you have 7 electrons and the atom is nitrogen so it becomes
_
:N:
.
Hope that helped
7 0
3 years ago
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