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Roman55 [17]
3 years ago
8

What is gas made up of?

Chemistry
1 answer:
horrorfan [7]3 years ago
6 0
Ethanol is the right answer headah boi
You might be interested in
Si se tiene 1mol de NO . cuantas moleculas de NO hay
kumpel [21]

if you have 1mol of NO. how many molecules of NO are there

Answer:

6.02 x 10²³ molecules

Explanation:

Given parameters:

Number of moles of NO = 1 mole

Unknown:

Number of molecules in NO;

Solution:

A mole of compound contains the Avogadro's number of particles.

  1 mole of a substance contains 6.02 x 10²³ molecules

So, 1 mole of NO contained 6.02 x 10²³ molecules

3 0
2 years ago
A 10.0 g pat of butter raise the water level in a graduated cylinder by 11.6 mL. What is the density of the butter
Nina [5.8K]

- formula for density is mass divided by volume

therefore density of butter = 10.0g divided by 11.6ml = 0.8620689 g/cm³ ≈ 0.862 g/cm³ (3sf)

8 0
3 years ago
For the following reaction, 4.31 grams of iron are mixed with excess oxygen gas . The reaction yields 5.17 grams of iron(II) oxi
natka813 [3]

<u>Answer:</u> The theoretical yield of iron (II) oxide is 5.53g and percent yield of the reaction is 93.49 %

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}       ....(1)

  • <u>For Iron:</u>

Given mass of iron = 4.31 g

Molar mass of iron = 53.85 g/mol

Putting values in above equation, we get:  

\text{Moles of iron}=\frac{4.31g}{53.85g/mol}=0.0771mol

For the given chemical reaction:

2Fe(s)+O_2(g)\rightarrow 2FeO(s)

By Stoichiometry of the reaction:

2 moles of iron produces 2 moles of iron (ii) oxide.

So, 0.0771 moles of iron will produce = \frac{2}{2}\times 0.0771=0.0771mol of iron (ii) oxide

Now, calculating the theoretical yield of iron (ii) oxide using equation 1, we get:

Moles of of iron (II) oxide = 0.0771 moles

Molar mass of iron (II) oxide = 71.844 g/mol

Putting values in equation 1, we get:  

0.0771mol=\frac{\text{Theoretical yield of iron(ii) oxide}}{71.844g/mol}=5.53g

To calculate the percentage yield of iron (ii) oxide, we use the equation:

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

Experimental yield of iron (ii) oxide = 5.17 g

Theoretical yield of iron (ii) oxide = 5.53 g

Putting values in above equation, we get:

\%\text{ yield of iron (ii) oxide}=\frac{5.17g}{5.53g}\times 100\\\\\% \text{yield of iron (ii) oxide}=93.49\%

Hence, the theoretical yield of iron (II) oxide is 5.53g and percent yield of the reaction is 93.49 %

7 0
2 years ago
of the following warnings, which one refers to a chemical property of a substance? fragile flammable handle with care shake well
coldgirl [10]
Flammable is ur answer
6 0
3 years ago
Why would an atom become an ion?
crimeas [40]

Answer:

c

Explanation: correct me if im wrong

5 0
3 years ago
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