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3 years ago

Wes melted some cheese over some tortilla chips to make nachos.

Chemistry

1 answer:

natima [27]3 years ago

4 0

Answer:

Explanation:

Because the mass would stay the same and the flavor did not change and neither did the color so the shape is the only thing that changed

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A sample of an unknown compound has a percent composition of 52.14% carbon, 13.13% hydrogen, and 34.73% oxygen. Which compounds

Artemon [7]

<h3>Answer:</h3>

The two possible compounds are;

1) Dimethyl Ether H₃C--O--CH₃

2) Ethanol H₃C--CH₂--OH

<h3>Solution:</h3>

Step 1: Calculate Moles of each Element;

Moles of C = %C ÷ At.Mass of C

Moles of C = 52.14 ÷ 12.01

Moles of C = 4.341 mol

Moles of H = %H ÷ At.Mass of H

Moles of H = 13.13 ÷ 1.01

Moles of H = 13.00 mol

Moles of O = %O ÷ At.Mass of O

Moles of O = 34.73 ÷ 16.0

Moles of O = 2.170 mol

Step 2: Find out mole ratio and simplify it;

C H O

4.341 13.00 2.170

4.341/2.170 13.00/2.170 2.170/2.170

2 5.99 1

2 6 1

Hence, Empirical Formula = C₂H₆O

<h3>Result:</h3>

As the molecular mass of compound is not given therefore, we can assume and guess the empirical formula to be the molecular formula. Hence, possible compounds are,

1) Dimethyl Ether H₃C--O--CH₃

2) Ethanol H₃C--CH₂--OH

3 0

3 years ago

How many liters of hydrogen gas will be produced at STP from the reaction of 7.179×10^23 atoms of magnesium with 54.219g of phos

Alexeev081 [22]

Answer: The volume of hydrogen gas produced will be, 12.4 L

Explanation : Given,

Mass of $H_3PO_4$ = 54.219 g

Number of atoms of $Mg$ = $7.179\times 10^{23}$

Molar mass of $H_3PO_4$ = 98 g/mol

First we have to calculate the moles of $H_3PO_4$ and $Mg$ .

$\text{Moles of }H_3PO_4=\frac{\text{Given mass }H_3PO_4}{\text{Molar mass }H_3PO_4}$

$\text{Moles of }H_3PO_4=\frac{54.219g}{98g/mol}=0.553mol$

and,

$\text{Moles of }Mg=\frac{7.179\times 10^{23}}{6.022\times 10^{23}}=1.19mol$

Now we have to calculate the limiting and excess reagent.

The balanced chemical equation is:

$3Mg+2H_3PO_4\rightarrow Mg(PO_4)_2+3H_2$

From the balanced reaction we conclude that

As, 3 mole of $Mg$ react with 2 mole of $H_3PO_4$

So, 0.553 moles of $Mg$ react with $\frac{2}{3}\times 0.553=0.369$ moles of $H_3PO_4$

From this we conclude that, $H_3PO_4$ is an excess reagent because the given moles are greater than the required moles and $Mg$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $H_2$

From the reaction, we conclude that

As, 3 mole of $Mg$ react to give 3 mole of $H_2$

So, 0.553 mole of $Mg$ react to give 0.553 mole of $H_2$

Now we have to calculate the volume of $H_2$ gas at STP.

As we know that, 1 mole of substance occupies 22.4 L volume of gas.

As, 1 mole of hydrogen gas occupies 22.4 L volume of hydrogen gas

So, 0.553 mole of hydrogen gas occupies $0.553\times 22.4=12.4L$ volume of hydrogen gas

Therefore, the volume of hydrogen gas produced will be, 12.4 L

4 0

3 years ago

Water is a compound not a mixture. Justify this statement by giving two reasons.

Allushta [10]

Answer:

Water is a compound and not a mixture. The reasons are the following:

1) It is held tightly through bonds called chemical bonds which is the characteristic of compound and not mixture.

2) It cannot be separated by physical means but can be separated by chemical means.

7 0

3 years ago

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What mass of au is produced when 0.0500 mol of au2s3 is reduced completely with excess h2?

olga_2 [115]

The mass of Au is 19.7 g

The chemical reaction may be

Au₂S₃ + 3H₂ → 2Au + 3H₂S

1 mole of Au₂S₃ gives 2 mole of Au

Then 0.0500 mol of Au₂S₃ gives

0.0500 × 2 / 1

= 0.10 moles.

To find mass

Mass = moles × molar mass

Moles = 0.10.

Molar mass = 197 g

Mass = 0.10 × 197

= 19.7 g

Hence the mass of Au produces is 19.7 g

Learn more about mass on

brainly.com/question/24550995

#SPJ4

7 0

2 years ago

Dr. Maxwell performed several experiments which seem to indicate that eating chocolate is always bad for your health. How should

svetoff [14.1K]

D. They should try to reproduce Dr. Maxwell's research to verify his results

3 0

4 years ago

Read 2 more answers