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12345 [234]
3 years ago
10

How adding tin to copper makes the bronze alloy harder?

Chemistry
2 answers:
andrey2020 [161]3 years ago
8 0
It makes the bronze stronger and harder than either of the other two medals
nika2105 [10]3 years ago
4 0
The molecules are different sizes so they can’t move past each other in the structure.
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Which pair of elements are in the same period?Hg & PbLi & NaB & ClO & As
Alexeev081 [22]

Answer:

Hg Pb are in one, Li and B and O are in one, and NaCl are in one, As is alone

Explanation:

Periods are horizontal

Hope this helps!

4 0
2 years ago
Which describes an covalent bond?
Ilya [14]

Answer:

is there choices you have to pick from

Explanation:

or do you have to describe a covalent bond ?

8 0
3 years ago
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In a solution of a carbonated beverage the water is what? Solute, saturated, solvent or precipitate
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3 years ago
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3 years ago
For the following reaction, 4.07 grams of aluminum oxide are mixed with excess sulfuric acid. The reaction yields 10.4 grams of
torisob [31]

Answer:

Theoretical yield = 13.7 g

% yield =76 %

Explanation:

For Al_2O_3

Mass of Al_2O_3  = 4.07 g

Molar mass of Al_2O_3  = 101.96 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{4.07\ g}{101.96\ g/mol}

Moles\ of\ Al_2O_3= 0.0399\ mol

According to the reaction:

Al_2O_3+3H_2SO_4\rightarrow Al_2(SO_4)_3+3H_2O

1 mole of Al_2O_3  on reaction produces 1 mole of Al_2(SO_4)_3

So,  

0.0399 mole of Al_2O_3  on reaction produces 0.0399 mole of Al_2(SO_4)_3

Moles of Al_2(SO_4)_3  obtained = 0.0399 mole

Molar mass of Al_2(SO_4)_3 = 342.2 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

0.0399= \frac{Mass}{342.2\ g/mol}

Mass= 13.7\ g

<u>Theoretical yield = 13.7 g</u>

The expression for the calculation of the percentage yield for a chemical reaction is shown below as:-

\%\ yield =\frac {Experimental\ yield}{Theoretical\ yield}\times 100

Given , Values from the question:-

Theoretical yield = 13.7 g

Experimental yield = 10.4 g

Applying the values in the above expression as:-

\%\ yield =\frac{10.4}{13.7}\times 100

<u>% yield =76 %</u>

6 0
3 years ago
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