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NemiM [27]
3 years ago
13

VSEPR theory predicts an identical shape for all of the following, except:_______. A. NH_3 B. H_3O^+ C. BH_3 D. CH_3^+ E. All of

these choice same geometry.
Chemistry
1 answer:
Vikentia [17]3 years ago
4 0

Answer:

C. BH_3

Explanation:

The VSEPR is known as the valence shell electron pair repulsion theory. The VSEPR theory determines the total number of electron pairs (TEP) surrounding the central atom of a species. The TEP consists of the bond pairs (BP) and lone pairs (LP). In this model, all the electron pairs (like charges) will orient themselves in such a way as to minimize the electrostatic repulsion between them. These repulsions determine the geometry of the covalent bonds around the central atom.

In the options given, all the molecules have identical geometry except BH_3. This is as a result of the absence of a lone pair on the BH_3 compound.

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At the Henry's Law constant for carbon dioxide gas in water is . Calculate the mass in grams of gas that can be dissolved in of
Dvinal [7]

The question is incomplete, here is the complete question:

At 25°C Henry's Law constant for carbon dioxide gas in water is 0.031 M/atm . Calculate the mass in grams of gas that can be dissolved in 425. mL of water at 25°C and at a partial pressure of 2.92 atm. Round your answer to 2 significant digits.

<u>Answer:</u> The mass of carbon dioxide that can be dissolved is 1.7 grams

<u>Explanation:</u>

To calculate the molar solubility, we use the equation given by Henry's law, which is:

C_{CO_2}=K_H\times p_{CO_2}

where,

K_H = Henry's constant = 0.031M/atm

C_{CO_2} = molar solubility of carbon dioxide gas

p_{CO_2} = partial pressure of carbon dioxide gas = 2.92 atm

Putting values in above equation, we get:

C_{CO_2}=0.031M/atm\times 2.92 atm\\\\C_{CO_2}=0.0905M

To calculate the mass of solute, we use the equation used to calculate the molarity of solution:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

Given mass of carbon dioxide = ? g

Molar mass of carbon dioxide = 44 g/mol

Molarity of solution = 0.0905mol/L

Volume of solution = 425 mL

Putting values in above equation, we get:

0.0905mol/L=\frac{\text{Mass of carbon dioxide}\times 1000}{44g/mol\times 425}\\\\\text{Mass of solute}=\frac{44\times 425\times 0.0905}{1000}=1.7g

Hence, the mass of carbon dioxide that can be dissolved is 1.7 grams

8 0
3 years ago
Consider the following reaction. Zn(s) 2agno3(aq) --&gt; 2ag(s) zn(no3)2(aq)when 16. 2 g of silver was produced, _____ mole(s) o
Crazy boy [7]

The required amount of silver nitrate to produce 16.2g of silver is 25.48 grams.

<h3>What is the relation between mass & moles?</h3>

Relation between the mass and moles of any substance will be represented as:

n = W/M, where

  • W = given mass
  • M = molar mass

Moles of silver = 16.2g / 107.8g/mol = 0.15mol

From the stoichiometry of the given reaction it is clear that, same moles of silver nitrate is required to produce same moles of silver. So 0.15 moles of silver nitrate is required.

Mass of silver nitrate = (0.15mol)(169.87g/mol) = 25.48g

Hence required mass of silver nitrate is 25.48g.

To know more about mass & moles, visit the below link:

brainly.com/question/19784089

#SPJ4

5 0
2 years ago
The pressure on a 200 milliliter sample of CO2 (g) at constant temperature is increased from
balu736 [363]

The answer for the following problem is mentioned below.

  • <u><em>Therefore the final volume of the gas is 100 ml.</em></u>

Explanation:

 Given:

Initial pressure (P_{1}) = 600 mm of Hg

Final pressure (P_{2}) = 1200 mm of Hg

Initial volume (V_{1}) = 200 ml      

To find:

Final volume (V_{2})

We know;

According to the ideal gas equation,

    P × V = n × R × T

Where;

P represents the pressure of the gas

V represents the volume of the gas

n represents the no of moles of the gas

R represents the universal gas constant

T represents the temperature of the gas

So,

 From the above mentioned equation,

        P × V = constant

\frac{P_{1} }{P_{2} } = \frac{V_{1} }{V_{2} }

Where,

(P_{1}) represents the initial pressure of the gas

(P_{2}) represents the final pressure of the gas

(V_{1})  represents the initial volume of the gas

(V_{2})  represents the final volume of the gas

So;

\frac{600}{1200} = \frac{V_{2} }{200}    

V_{2} = 100 ml

<u><em>Therefore the final volume of the gas is 100 ml.</em></u>                                                                                                                                                                              

5 0
3 years ago
How many moles are 21.67 L of NH4CI?<br> Type your answer...
NNADVOKAT [17]

Answer:

0.967mole

Explanation:

Given parameters:

Volume of NH₄Cl  = 21.67L

Unknown:

Number of moles  = ?

Solution:

We assume that the volume was taken at standard temperature and pressure,

 Then;

  Number of moles  = \frac{volume }{22.4L}  

 Number of moles  = \frac{21.67}{22.4}   = 0.967mole

6 0
2 years ago
I NEED HELP PLEASE, THANKS! :)
marin [14]

Answer:

\large \boxed{1.447 \times 10^{23}\text{ molecules Cu(OH)}_{2 }}

Explanation:

1. Calculate the moles of copper(II) hydroxide

\text{Moles of Cu(OH)}_{2} = \text{23.45 g Cu(OH)}_{2} \times \dfrac{\text{1 mol Cu(OH)}_{2}}{\text{97.562 g Cu(OH)}_{2}} = \\\\\text{0.240 36 mol Cu(OH)}_{2}

2. Calculate the molecules of copper(II) hydroxide

\text{No. of molecules} = \text{0.240 36 mol Cu(OH)}_{2} \times \dfrac{6.022 \times 10^{23}\text{ molecules Cu(OH)}_{2}}{\text{1 mol Cu(OH)}_{2}}\\\\= 1.447 \times 10^{23}\text{ molecules Cu(OH)}_{2}\\\text{The sample contains $\large \boxed{\mathbf{1.447 \times 10^{23}}\textbf{ molecules Cu(OH)}_{\mathbf{2}}}$}

6 0
3 years ago
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