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3 years ago

Need help plzz

Chemistry

1 answer:

frozen [14]3 years ago

5 0

Answer: B. Magnification.

Yes you are absolutely right. Although Enlargement and Magnification have similar meanings, the correct term used for objects that get larger in a microscope is called magnification. Magnification in a microscope refers to the enlargement of the object that is being observed in the microscope.

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ziro4ka [17]

Answer:

The answer is Protein.

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3 years ago

What is the oxidation state of cl in hclo4?

Irina-Kira [14]

There is 1 H atom: (1)(+1) = +1 The oxidation number of O is -2. There are 4 O atoms here: (4)(-2) = -8 So the oxidation state of Cl is +7.

NOTE: The maximum positive oxidation number for chlorine is +7, the same as its group number (VII).

3 0

3 years ago

Read 2 more answers

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

3 years ago

Hellllpppp What is propane's condensed structural formula?

mrs_skeptik [129]

Answer,

Propane's condensed structural formula is CH3 CH2 CH3.

Hope This Helps :-)

7 0

3 years ago

The mass spectra of alcohols often fail to exhibit detectable M peaks but instead show relatively large ________ peaks.

nirvana33 [79]

Answer: M-18

Explanation:

The mass spectra of alcohols often fail to exhibit detectable M peaks but instead show relatively large __M-18___ peaks.

Mass spectroscopy is used to determine the molecular mass and molecular formula of a sample.

When the mass spectra of alcohols do not show detectable M peaks, they show relatively large M-18 peaks.

6 0

3 years ago