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3 years ago

What is gas made up of?

Chemistry

1 answer:

horrorfan [7]3 years ago

6 0

Ethanol is the right answer headah boi

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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]

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

Explanation:

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

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

For Iron:

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:

Explanation: correct me if im wrong

5 0

3 years ago