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2 years ago

Q1. The equation for the reaction between sulfur dioxide and oxygen is shown.

1 answer:

3 0

The mole fraction of sulfur trioxide in the equilibrium mixture is 0.353.
Hence option (B) is the correct answer.

<h3>What is mole fraction ?</h3>

The ratio of the number of moles of one component of a solution or other mixture to the total number of moles representing all of the components.

We have to use algebra here,

Because in the equation $O_2$ has a stoichometry of 1, the other have 2,

let $O_2$ = x

You started with 2 moles, so the moles of $O_2$ at equilibrium will be 2 - X

$SO_3$ has a stoichiometry of 2 compared to $O_2$ , so will be 2X

( not minus from anything as you started with no moles of $SO_3$ )

And then $SO_2$ will also be 2X as it’s stoichiometry is 2, but as you started with 2 moles it will be 2-2X

If you add these in an equation to get total moles it’s

2 - 2X + 2 - X + 2X = 3.4 (total given)

and then gathering together becomes 4-X = 3.4

so,

4 = 3.4 + X

so,

x = 0.6

Therefore,

the moles of $SO_3$ = 2 x 0.6 = 1.2

mole fraction = moles of the gas / total moles of gas

mole fraction = 1.2 / 3.4 = 0.353

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Write the full electron configuration of the Period 2 element with the following successive IEs (in kJ/mol):

Julli [10]

Answer:

Boron (B) is the element whose IE matches with our data.

Electronic Configuration of boron: $1s^22s^22p^1$

Explanation:

Ionization Energy (IE):

It is the minimum amount of energy which is required to remove the lose electron. If the electron is closer to the nucleus then greater amount of energy is required to remove the electron.

If we look from left to right in a period, ionization energy increases due stability of valance shell.

From the data given to us:

IE₁ = 801

IE₂ = 2427

IE₃ = 3659

IE₄ = 25,022

IE₅ = 32,822

Boron (B) is the element whose IE matches with our data.

Electronic Configuration of boron: $1s^22s^22p^1$

Boron has 5 electrons (3 in valance shell) that's why it has 5 Ionization Energies.

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3 years ago

Determine which of the following statement is correct when the equilibrium constant K for a certain reaction is 10 at 298 K and

aev [14]

Answer:

4. The reaction is spontaneous at any temperatures if the standard entropy of reaction is positive.

Explanation:

Equilibrium constant decreases on increasing the temperature . So the reaction appears to be exothermic . In other words

ΔH is negative .

Δ G = ΔH - TΔS

If ΔS is positive , second term is negative . ΔH is negative so the RHS of the equation is negative at all temperatures . Hence Δ G of the reaction is negative . So reaction is spontaneous at any temperature.

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3 years ago

Why factory waste should be neutralized before disposing it into the water bodies?

Fudgin [204]

Explanation:

Factory wastes are usually acidic and they pose serious environmental challenges.

If an untreated acidic waste is discharged into the river, the acidity of the river increases and this is toxic to life in the water.

On land, the acid can enter into the soil and prevent plant growth.

Acid discharge can enter the groundwater system and render it unfit for use.

Bases and a couple of additives are used to remove acidity from factory wastes before they are discharged.

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3 years ago

1. list at least two possible sources of error from the experiment. would these errors result in an overestimation or an underes

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An error in estimation could arise owing to;

1) Inaccurate measurement of the volumes of the solutions

2) When the reaction vessels are not properly cleaned

<h3>What is error in an experiment?</h3>

Error could occur in an experiment when values are misread. The error could be random error or a systematic error.

The major ways in which an error can occur in the estimation of concentration of acetic acid in the vinegar are;

1) Inaccurate measurement of the volumes of the solutions

2) When the reaction vessels are not properly cleaned

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2 years ago

Water can act as both an acid and a base in an ionization reaction to form (H) and OH ions.

matrenka [14]

Sorry I need points :)

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3 years ago

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