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adoni [48]
3 years ago
7

In an anatomy class, a student has been learning about the bones of the body. While taking a test, he needs to identify the ster

num, which is a thin, flat bone with bumpy edges.
Which bone is the sternum?
Chemistry
2 answers:
liberstina [14]3 years ago
4 0

Answer:

No doubt the answer is (A

Explanation:

I took the quiz! :D

storchak [24]3 years ago
3 0

Answer:

The term “flat bone” is somewhat of a misnomer because, although a flat bone is typically thin, it is also often curved. Examples include the cranial (skull) bones, the scapulae (shoulder blades), the sternum (breastbone), and the ribs. Flat bones serve as points of attachment for muscles and often protect internal organs.

HOPE THIS HELPS!!! :D

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A rocks or a desk would be molecular solid. Ex. gas is not a molecular solid. 
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4 years ago
When the following equation is balanced with lowest whole-number coefficients, what is the coefficient for NO(g)? ___NH3(g) + __
inn [45]

Answer:

Coefficient in front of the NO in the balanced equation - 4

Explanation:

The unbalanced reaction is shown below as:-

NH_3+O_2\rightarrow NO+H_2O

On the left hand side,  

There are 1 nitrogen atom and 3 hydrogen atoms and 3 oxygen atoms

On the right hand side,  

There are 1 nitrogen atom and 2 hydrogen atoms and 2 oxygen atoms

Thus,  

Right side, H_2O must be multiplied by 6 and NO by 4

Left side, O_2 is multiplied by 5 and NH_3 by 4 so to balance the whole reaction.

Thus, the balanced reaction is:-

4NH_3+5O_2\rightarrow 4NO+6H_2O

<u>Coefficient in front of the NO in the balanced equation - 4</u>

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3 years ago
If you were testing how well different laundry soaps clean your clothes the control group would be​
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4 years ago
A three-step process for producing molten iron metal from Fe2O3 is: 3Fe2O3 + CO → 2Fe3O4 + CO2 Fe3O4 + CO → 3FeO + CO2 FeO + CO
miskamm [114]

Answer:

There is 100.4652 kg of iron produced from 390 kg of Fe2O3

Explanation:

<u>Step 1</u>: Given data

3Fe2O3 + CO → 2Fe3O4 + CO2

Fe3O4 + CO → 3FeO + CO2

FeO + CO → Fe + CO2

Mass of Fe2O3 = 390 kg = 390000 grams

Molar mass of Fe2O3 = 159.69 g/moles

<u>Step 2: </u>Calculate moles of Fe2O3

Moles of Fe2O3 = mass of Fe2O3 / Molar mass of Fe2O3

Moles of Fe2O3 = 390000 grams / 159.69 g/moles = 2442.2 moles

<u>Step 3</u>: Calculate expected moles of Fe3O4

In the first equation, for 3 moles of Fe2O3 consumed ,we get 2 moles of Fe3O4. The mole ratio is 3:2

This means if we consume 2442.2 moles of Fe2O3, there will be produced 2/3 * 2442.2 = 1628.2 moles of Fe3O4

Since the yield for the step is only 84.6 %

This will be 0.846 * 1628.2 = 1377.4 moles of Fe3O4

<u>Step 4:</u> Calculate expected moles of FeO

In the second equation, for 1 mole of Fe3O4 consumed, there is produced 3 moles of FeO

This means for 1377.4 moles of Fe3O4 consumed, there is 3*1377.4 = 4132.2 moles of FeO produced

Since the yield for the step is only 50.8%

This will be 0.508 * 4132.2 = 2099.2 moles of FeO

<u>Step 5:</u> Calculate expected moles of Fe

In the third equation, for 1 mole of FeO consumed, there is produced 1 mole of Fe.

This means for 2099.2 moles of FeO consumed, there is also 2099.2 moles of Fe produced

Since the yield is only 85.7%

This will be 0.857 * 2099.2 = 1799 moles of Fe

<u>Step 6:</u> Calculate mass of Fe

Mass of Fe = moles of Fe * Molar mass of Fe

Mass of Fe = 1799 moles of Fe * 55.845 g/moles = 100465.2 grams = 100.4652 kg of Fe

There is 100.4652 kg of iron produced from 390 kg of Fe2O3

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