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3 years ago

Give the following for SO2 and BrF5:

Chemistry

1 answer:

frosja888 [35]3 years ago

6 0

Answer:

The given molecules are SO2 and BrF5.

Explanation:

Consider the molecule SO2:

The central atom is S.

The number of domains on S in this molecule is three.

Domain geometry is trigonal planar.

But there is a lone pair on the central atom.

So, according to VSEPR theory,

the molecular geometry becomes bent or V-shape.

Hybridization on the central atom is

$sp^{2}$ .

Consider the molecule BrF5:

The central atom is Br.

The number of domains on the central atom is six.

Domain geometry is octahedral.

But the central atom has a lone pair of electrons.

So, the molecular geometry becomes square pyramidal.

The hybridization of the central atom is $sp^{3} d^{2}$ .

The shapes of SO2 and BrF5 are shown below:

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A fluorine atom has 9 positive charge,9 negative charges and a mass of 19. Describe the structure of its atom.

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The atomic structure of the atom contains 9 positively charged particles (protons) and 10 neutrally charged particles (neutrons) in the center of the atom in a clump called the nucleus. Those 9 negatively charged particles (electrons) are moving around outside of the nucleus.
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How many moles of KNO3 are in 500 mL of 2. 0 M KNO3? mol KNO3.

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The moles can be defined as the mass of the substance with respect to molar mass. The moles of potassium nitrate is 1 mol.

<h3>How to calculate moles of a substance?</h3>

The moles of a compound can be calculated from:

$\rm Moles=\dfrac{Mass}{Molar\;mass}$

The molarity can be defined as the moles of solute in a liter of solution.

The molarity can be expressed as:

$\rm Molarity=\dfrac{Moles\;\times\;1000}{Volume\;(mL)}$

The molarity of potassium nitrate solution is 2 M, and the volume is 500 mL.

The moles of potassium nitrate is given as:

$\rm 2\;M=\dfrac{Moles\;\times\;1000}{500\;mL}\\ Moles=\dfrac{2\;\times\;500}{1000}\;mol\\ Moles=1\;mol$

The moles of potassium nitrate in 2 M, 500 mL solution are 1 mol.

Learn more about moles, here:

brainly.com/question/15209553

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2 years ago

Iron(III) oxide and hydrogen react to form iron and water, like this: Fe_2O_3(s) + 3H_2(g) rightarrow 2Fe(s) + 3H_2O(g) At a cer

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Complete Question

The complete question is shown on the first uploaded image

Answer:

The equilibrium constant is $K_c= 2.8*10^{-4}$

Explanation:

From the question we are told that

The chemical reaction equation is

$Fe_{2} O_{3}_{(s)} + 3H_{2}_{(g)} -----> 2Fe_{(s)} + 3H_{2} O_{(g)}$

The voume of the misture is $V_m = 5.4L$

The molar mass of $Fe_{2} O_{3}_{(s)}$ is a constant with value of $M_{Fe_{2} O_{3}_{(s)} } = 160g/mol$

The molar mass of $H_{2}_{(g)}$ is a constant with value of $H_2 = 2g/mol$

The molar mass of $H_{2}O$ is a constant with value of $H_2O = 18g/mol$

Generally the number of moles is mathematically given as

$No \ of \ moles \ = \frac{mass}{molar\ mass}$

For $Fe_{2} O_{3}_{(s)}$

$No \ of\ moles = \frac{3.54}{160}$

$= 0.022125 \ mols$

For $H_{2}$

$No \ of\ moles = \frac{3.63}{2}$

$= 1.815 \ mols$

For $H_{2}O$

$No \ of\ moles = \frac{2.13}{18}$

$= 0.12 \ mols$

Generally the concentration of a compound is mathematicallyrepresented as

$Concentration = \frac{No \ of \ moles }{Volume }$

For $Fe_{2} O_{3}_{(s)}$

$Concentration[Fe_2 O_3] = \frac{0.222125}{5.4}$

$= 4.10*10^{-3}M$

For $H_{2}$

$Concentration[H_2] = \frac{1.815}{5.4}$

$= 0.336M$

For $H_{2}O$

$Concentration [H_2O] = \frac{0.12}{5.4}$

$= 0.022M$

The equilibrium constant is mathematically represented as

$K_c = \frac{[concentration \ of \ product]}{[concentration \ of \ reactant ]}$

Considering $H_2O \ for \ product$

And $H_2 \ for \ reactant$

At equilibrium the

$K_c = \frac{0.022}{0.336}$

$K_c= 2.8*10^{-4}$

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3 years ago

Why can't all mixtures be classified as solutions?

natulia [17]

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Homogeneous solution of salt and water can be separated with heating (evaporating the water).

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