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sleet_krkn [62]
2 years ago
11

How is an atomic radius measured?

Chemistry
1 answer:
Lelu [443]2 years ago
4 0

Answer:

The radius of an atom can only be found by measuring the distance between the nuclei of two touching atoms, and then halving that distance.

Explanation:

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Water quality tests show the presence of a single heavy metal in the drinking water pulled from a local river. Residents are suf
just olya [345]

Answer:

One metal causes a chronic effect, compared to the other

Explanation:

because the question only said ONE is the same, didn't they? so that would mean that not all the metals are the same for both towns

4 0
3 years ago
Which element is the first element in group 13 of the periodic table of elements?​
joja [24]

Answer:

Boron

Explanation:

8 0
3 years ago
Read 2 more answers
A 13.00 g sample of a compound contains 4.15 g potassium (k), 3.76 g chlorine (cl), and oxygen (o). calculate the empirical form
MrRissso [65]

To solve this problem, let us all convert the mass of each element into number of moles using the formula:

moles = mass / molar mass

Where,

molar mass K = 39.10 g / mol

<span>molar mass Cl = 35.45 g / mol</span>

molar mass O = 16 g / mol

<span>and mass O = 13 g – 4.15 g – 3.76 g  = 5.09 g</span>

 

moles K = 4.15 g / (39.10 g / mol) = 0.106 mol

<span>moles Cl = 3.76 g / (35.45 g / mol) = 0.106 mol</span>

moles O = 5.09 g / (16 g / mol) = 0.318 mol

 

The ratio becomes:

0.106 K: 0.106 Cl: 0.318 O

We divide all numbers with the smallest number, in this case 0.106. This becomes:

K: Cl: 3O

 

Therefore the empirical formula is:

KClO_{3}

7 0
2 years ago
What are isotopes?
Elis [28]

Answer:

B

Explanation:

6 0
2 years ago
Read 2 more answers
Determine the theoretical maximum moles of hydroquinone, , that could be produced in this experiment. The reactant, quinone, is
dedylja [7]

Answer:

Theoretical maximum moles of hydroquinone: 0.2167 mol.

Explanation:

Hello,

In this case, the undergoing chemical reaction is like:

Quinone\rightarrow Hydroquinone

In such a way, since the molar mass of quinone is 108.1 g/mol and it is in a 1:1 molar ratio with hydroquinone, we can easily compute the theoretical maximum moles of hydroquinone by stoichiometry:

n_{hydroquinone}=23.4g\ quinone*\frac{1mol\ quinone}{108.1 g\ quinone}*\frac{1mol\ hydroquinone}{1mol\ quinone}  \\\\n_{hydroquinone}=0.2167mol

Clearly, this is the theoretical yield which in grams is:

m_{hydroquinone}=0.2167mol*\frac{110.11g}{1mol} =23.84g

Which allows us to compute the percent yield as well since the obtained mass of the product is 13.0 g:

Y=\frac{13.0g}{23.84g}*100\%=54.5\%

Best regards.

8 0
2 years ago
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