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2 years ago

Use the portion of the periodic table shown below to answer the questions.

Chemistry

1 answer:

Bingel [31]2 years ago

4 0

The two elements that have the same properties as sodium are potassium and rubidium .

<h3>What is periodic table?</h3>

The periodic table is an arrangement of the elements in order of increasing atomic number.

From the list, the two elements that have the same properties as sodium are potassium and rubidium .

Proton has an atomic number of 20 and a mass number of 40. The number of electrons is the same as the number of protons. Given that the atomic number is the number of protons present, we have 20 electrons and 20 protons.

Number of neutrons = Mass number - Number of protons

= 40 - 20 = 20 neutrons

Learn more about periodic table:brainly.com/question/11155928

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Explain why are hydrogen and oxygen considered wheares water as a compound

mestny [16]

Hydrogen and oxygen are different elements ...
but when two or more elements combine... it is known as a compound.. hence hydrogen and oxygen together form a compound

6 0

3 years ago

Exposing a 250 mL sample of water at 20.∘C to an atmosphere containing a gaseous solute at 27.59 kPa resulted in the dissolution

ElenaW [278]

Answer : The solubility of this gaseous solute will be, $5.18\times 10^{-5}g/mL$

Explanation :

First we have to calculate the concentration of solute.

$\text{Concentration of solute}=\frac{Mass}{Volume}=\frac{4.51\times 10^{-3}g}{250mL}=1.80\times 10^{-5}g/mL$

Now we have to calculate the Henry's law constant.

Using Henry's law :

$C=k_H\times p$

where,

C = concentration of solute = $1.80\times 10^{-5}g/mL$

p = partial pressure = 27.59 kPa

$k_H$ = Henry's law constant = ?

Now put all the given values in the above formula, we get:

$1.80\times 10^{-5}g/mL=k_H\times (27.59kPa)$

$K_H=6.52\times 10^{-7}g/mL.kPa$

Now we have to calculate the solubility of this gaseous solute when its pressure is 79.39 kPa.

$C_{(79.39kPa)}=k_H\times p$

$C_{(79.39kPa)}=(6.52\times 10^{-7}g/mL.kPa)\times (79.39kPa)$

$C_{(79.39kPa)}=5.18\times 10^{-5}g/mL$

Therefore, the solubility of this gaseous solute will be, $5.18\times 10^{-5}g/mL$

7 0

3 years ago

How many moles are equal to 83.4 L of O2?

ladessa [460]

Answer:

$3.72mol$

Explanation:

Hello,

In this case, we consider that at STP conditions (273 K and 1 atm) we know that the volume of 1 mole of a gas is 22.4 L, thereby, for 83.4 L, the resulting moles are:

$22.4L\rightarrow 1mol\\83.4L\rightarrow X\\X=\frac{83.4L*1mol}{22.4L}=3.72mol$