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Sergio039 [100]
3 years ago
12

What is the atomic number of iron oxide?

Chemistry
2 answers:
Irina-Kira [14]3 years ago
5 0

Answer:

26. Hemoglobin is a tetramer that consists of four polypeptide chains. Each monomer contains a heme group in which an iron ion is bound to oxygen.

Explanation:

lisov135 [29]3 years ago
5 0

Answer:

26. (I think.)

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True or false: Halogens are very stable because they have a full outer shell of 8
STALIN [3.7K]

Answer:

True

Explanation:

Halogens are very stable because they have a full outer shell of 8

true or false?

Brainiest plz and hope this answer helped let me know if you need any more help I am glad to help!

It's true!

8 0
2 years ago
Ten lab safety rules
Bogdan [553]
Don't touch your eyes.

Never taste-test unless the teacher tells you to.

Do not touch anything without directions.

Wear safety goggles. 

Wash your hands after each experiment.

Wear proper lab clothes.

Do not mishandle lab equipment.

Clean up your workplace.

Act serious; no horseplay!

Report accidents to the teacher right away!


Have a great day, scholar! 
4 0
3 years ago
Which energy conservation takes place when a solar cell
sp2606 [1]

Answer:

Its science and cells

Explanation:

5 0
3 years ago
Read 2 more answers
Salicylic acid will reach with methanol (CH3OH), and form methyl salicylate. This is another esterification reaction, only this
allochka39001 [22]

Answer:

C7H603   +    CH3OH --> C8H803  + H2O

Balanced equation with corresponding stoichiometric numbers.

Explanation:

the salicylic acid, also called aspirin, when reacting with methanol produced an irreversible reaction giving methyl salicylate and water

8 0
3 years ago
Consider the reaction 2CO * O2 —> 2 CO2 what is the percent yield of carbon dioxide (MW= 44g/mol) of the reaction of 10g of c
Arturiano [62]

Answer:

Y = 62.5%

Explanation:

Hello there!

In this case, for the given chemical reaction whereby carbon dioxide is produced in excess oxygen, it is firstly necessary to calculate the theoretical yield of the former throughout the reacted 10 grams of carbon monoxide:

m_{CO_2}^{theoretical}=10gCO*\frac{1molCO}{28gCO}*\frac{2molCO_2}{2molCO}  *\frac{44gCO_2}{1molCO_2}\\\\ m_{CO_2}^{theoretical}=16gCO_2

Finally, given the actual yield of the CO2-product, we can calculate the percent yield as shown below:

Y=\frac{10g}{16g} *100\%\\\\Y=62.5\%

Best regards!

8 0
2 years ago
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