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1 month ago

At standard pressure the boiling point of an unsaturated nano3(aq) solution increases when

Chemistry

2 answers:

VMariaS [2.9K]1 month ago

5 0

The answer is 4.

Anarel [2.9K]1 month ago

4 0

When dealing with an unsaturated NaNO3(aq) solution at standard pressure, the boiling point increases when...

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"A sample of silicon has an average atomic mass of 28.084amu. In the sample, there are three isotopic forms of silicon. About 92

lorasvet [2795]

Answer: The percentage abundance for $_{14}^{30}\textrm{Si}$ isotope is 3.09 %.

Explanation:

The average atomic mass of an element is calculated by taking the sum of the masses of all isotopes weighted by their respective natural fractional abundances.

To compute average atomic mass, the following formula is applied:

$\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i$ .....(1)

From the information provided:

Let the fractional abundance for $_{14}^{28}\textrm{Si}$ isotope be 'x'

For $_{14}^{28}\textrm{Si}$ isotope:

Mass of $_{14}^{28}\textrm{Si}$ isotope = 27.9769 amu

Percentage abundance of $_{14}^{28}\textrm{Si}$ isotope = 92.22 %

Fractional abundance for $_{14}^{28}\textrm{Si}$ isotope = 0.9222

For $_{14}^{29}\textrm{Si}$ isotope:

Mass of $_{14}^{28}\textrm{Si}$ isotope = 28.9764 amu

Percentage abundance for $_{14}^{28}\textrm{Si}$ isotope = 4.68%

Fractional abundance of $_{14}^{28}\textrm{Si}$ isotope = 0.0468

For $_{14}^{30}\textrm{Si}$ isotope:

Mass of $_{14}^{30}\textrm{Si}$ isotope = 29.9737 amu

Fractional abundance for $_{14}^{30}\textrm{Si}$ isotope = x

The average atomic mass of silicon is 28.084 amu

By inserting these values into equation 1, we derive:

$28.084=[(27.9769\times 0.9222)+(28.9764\times 0.0468)+(29.9737\times x)]\\\\x=0.0309$

To convert this fractional abundance into a percentage, multiply by 100:

$\Rightarrow 0.0309\times 100=3.09\%$

This shows that the percentage abundance for $_{14}^{30}\textrm{Si}$ isotope is 3.09 %.

6 0

2 months ago

What do you do with unused (excess) chemicals that are taken from reagent bottles?

Alekssandra [3086]

Unused chemicals should never be returned to their original containers, as this could lead to contamination. The leftover chemicals should be disposed of in the appropriate waste bin. If there is uncertainty about the procedure, consult your teacher.

4 0

2 months ago

If 1.0 mole of CH4 and 2.0 moles of Cl2 are used in the reaction CH4 + 4Cl2 => CCl4 + 4HCl then which of these statements is

lions [2927]

Answer:

B,C,D

Explanation:

The quantity of CCl4 produced is contingent on the amount of CH4 used in a 1:1 ratio. Given that there are twice as many moles of Cl2 compared to CH4, some Cl2 will remain unreacted. To fully utilize all Cl2, additional CH4 must be introduced into the reaction.

4 0

1 month ago

Activity 1: My Incompleteness, Complete Me. Fill in the Punnett squares with the correct genotypes based on the key pictures tha

Alekssandra [3086]

I hope you can decipher it and that it's also accurate. Wishing you all the best.

8 0

2 months ago

Determine the type of each chemical equation describing a precipitation reaction. C a 2 + ( a q ) + S O 4 2 − ( a q ) ⟶ C a S O

lorasvet [2795]

Answer:

C a B r 2 ( a q ) + N a 2 S O 4 ( a q ) ⟶ 2 N a B r ( a q ) + C a S O 4 ( s )

Explanation:

A precipitation reaction involves a displacement process where a solid precipitate forms. This precipitate, being solid, is distinct from the other products and can be separated.

C a 2 + ( a q ) + S O 4 2 − ( a q ) ⟶ C a S O 4 ( s )

This equation is incorrect as it results in only C a S O 4.

C a B r 2 ( a q ) + N a 2 S O 4 ( a q ) ⟶ 2 N a B r ( a q ) + C a S O 4 ( s )

This is the proper reaction where C a S O 4 precipitate is produced.

C a 2 + ( a q ) + 2 B r − ( a q ) + 2 N a + ( a q ) + S O 4 2 − ( a q ) ⟶ 2 N a + ( a q ) + 2 B r − ( a q ) + C a S O 4 ( s )

This equation illustrates the ionic details of the precipitation reaction.

8 0

2 months ago