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Troyanec [42]
3 years ago
14

10 points

Chemistry
1 answer:
artcher [175]3 years ago
7 0
C. arteries, veins, capillaries
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Lewis dot structure of PSI3 with minimized formal charges
vredina [299]

We need to know how many valence electrons are present in a given molecule in order to determine its Lewis dot structure.

<h3>What is Lewis dot structure?</h3>

Lewis dot structure is defined as the visual representation of atoms' electrons using a diagram. It describe the bonds that exist between a molecule's lone pairs of electrons and its atoms.

A lone pair of electrons on the atom with the formal charge of 1- can typically be converted into a bonding pair that is shared with the atom that has the formal charge of 1+ in order to reduce the formal charges when they are present.

Thus, we need to know how many valence electrons are present in a given molecule in order to determine its Lewis dot structure.

To learn more about Lewis dot structure, refer to the link below:

brainly.com/question/20300458

#SPJ1

3 0
2 years ago
Freé point<br><img src="https://tex.z-dn.net/?f=%20%5C%3A%20%20%5C%3A%20%20%5C%3A%20%20%5C%3A%20%20%5C%3A%20%20%5C%3A%20" id="Te
gladu [14]

Answer

Tq so much.

Pls follow me and Mark as brainliest Plsssssssss

5 0
3 years ago
Read 2 more answers
Ammonia (NH3) is widely used as a fertilizer
ratelena [41]

Answer:

82.28g

Explanation:

Given parameters:

Number of moles of hydrogen gas = 7.26 moles

Unknown:

Amount of ammonia produced = ?

Solution:

We have to write the balanced equation first.

              N₂    +   3H₂    →    2NH₃

Now, we work from the known to the unknown;

   

                  3 moles of H₂ will produce 2 moles of NH₃

                7.26 mole of H₂ will produce \frac{7.26 x 2}{3}  = 4.84 moles of NH₃

Molar mass of NH₃ = 14 + 3(1) = 17g/mol

Mass of NH₃  = number of moles  x molar mass = 4.84 x 17 = 82.28g

3 0
3 years ago
Ammonia (NH3) reacts with oxygen (O2) to produce nitrogen monoxide (NO) and water (H2O). Write and balance the chemical equation
bekas [8.4K]

Answer:

There is 1.6 L of NO produced.

Explanation:

I assume you have an excess of NH3 so that O2 is the limiting reagent.

<u>Step 1:</u> Data given

2.0 liters of oxygen reacts with ammonia

<u>Step 2:</u> The balanced equation

4NH3 + 5O2 → 4NO + 6H2O

For 4 moles of NH3, we need 5 moles of O2 to produce 4 moles of NO and 6 moles of H2O

Consider all gases are kept under the same conditions for pressure and temperature, we can express this mole ratio in terms of the volumes occupied by each gas.

This means:  when the reaction consumes  4  liters of ammonia (and 5 liters of oxygen) it produces  4  liters of nitrogen  monoxide

Now, when there is 2.0 liters of oxygen consumed, there is 4/2.5 = 1.6 L of nitrogen monoxide produced.

There is 1.6 L of NO produced.

4 0
4 years ago
When 0.215 mol of a gas is placed into a 34.25 mL container at 125.0°C, 1
horrorfan [7]

Answer:

205.12 atm

Explanation:

Using the ideal gas law equation:

PV = nRT

Where;

P = pressure (atm)

V = volume (L)

R = 0.0821 Latm/perK)

T = temperature (K)

n = number of moles (mol)

According to the information in this question;

P = ?

V = 34.25 mL = 34.25 ÷ 1000 = 0.03425L

n = 0.215 mol

T = 125.0°C = 125 + 273 = 398K

Using PV = nRT

P = nRT ÷ V

P = (0.215 × 0.0821 × 398) ÷ (0.03425)

P = 7.025 ÷ 0.03425

P = 205.12 atm

8 0
3 years ago
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