All categories

4 years ago

How much iron can be recovered from 25 grams of Fe2O3

Chemistry

2 answers:

Scilla [17]4 years ago

3 0

25.0g of Fe2O3. 2(55.8)g+3(16.0)g=159.9g. 2(55.8)g/159.6g•100%= 69.9%. 69.9%/100%•25.0g=17.5g of iron recovered

Radda [10]4 years ago

3 0

Answer: The mass of iron recovered is 17.5 grams

Explanation:

We are given a chemical compound having chemical formula of $Fe_2O_3$

We know that:

Molar mass of iron (III) oxide = 159.7 g/mol

Mass of iron = 55.8 g/mol

We are given:

Mass of iron (III) oxide = 25 g

To calculate the mass of iron recovered in given amount of iron (III) oxide, we use unitary method:

From 159.7 grams of iron (III) oxide, mass of iron recovered is $(2\times 55.8)g$

So, from 25 grams of iron (III) oxide, mass of iron recovered will be $\frac{(2\times 55.8)}{159.7}\times 25=17.5g$

Hence, the mass of iron recovered is 17.5 grams

You might be interested in

What is the answer to this question

irina [24]

I am going to say D and C.

3 0

3 years ago

During science lab, Carl notices that when he adds water to his solid sample of anhydrous copper

Bond [772]

Answer:

The dissociation of copper sulfate into ions is an exothermic chemical reaction that releases heat into the surroundings.

Explanation:

Some of the potential energy stored in the solid sample of anhydrous copper sulfate is released as heat as the sample dissolves and dissociates into ions in the water. This is due to the large lattice energy of the crystalline copper sulfate.

hope this helps

4 0

3 years ago

Which of the following words means "the thing from which something else comes"?

swat32

Answer:

b. source

Explanation:

The source is where something comes from. i.e. The source of sunlight is the sun.

7 0

4 years ago

Read 2 more answers

A student measures out exactly 0.105 g of salicylic acid and runs the experiment as dictated in the lab manual. They obtain 0.11

scoray [572]

Answer: The percent yield of the reaction is 8.10 %.

Explanation:

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

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

Given mass of salicylic acid = 0.105g

Molar mass of salicylic acid = 138.12 g/mol

Putting values in equation 1, we get:

$\text{Moles of salicylic acid}=\frac{0.105g}{138.12g/mol}=0.0079mol$

The chemical equation for the formation of aspirin from salicylic acid follows:

$\text{Salicylic acid + Acetic anhydride}\rightarrow \text{Aspirin + Acetic acid}$

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin

So, 0.0076 moles of salicylic acid will produce = $\frac{1}{1}\times 0.0076=0.0076mol$ of aspirin

Now, calculating the mass of aspirin from equation 1, we get:

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.0076 moles

Putting values in equation 1, we get:

$0.0076mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=(0.0076mol\times 180.16g/mol)=1.37g$

To calculate the percentage yield of aspirin, we use the equation:

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

Experimental yield of aspirin = 0.111 g

Theoretical yield of aspirin = 1.37 g

Putting values in above equation, we get:

$\%\text{ yield of aspirin}=\frac{0.111g}{1.37g}\times 100\\\\\% \text{yield of aspirin}=8.10\%$

Hence, the percent yield of the reaction is 8.10 %.

6 0

3 years ago

After a lightning storm, the Rodriguez family notices the TV no longer works.

rosijanka [135]

The answer is B. have a good day! :)

8 0

3 years ago