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3 years ago

What does a net ionic equation show about a reaction

Chemistry

1 answer:

AVprozaik [17]3 years ago

6 0

Answer:

A net ionic equation shows only the chemical species that are involved in a reaction, while a complete ionic equation also includes the spectator ions.

Brainlist pls!

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I don’t really have a question... and my teacher says I need to give one related to this reading above :/

irinina [24]

Answer:

Just say I wonder why teachers give homework :/

Explanation:

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4 years ago

If you made a three-dimensional model of an atom and its nucleus, how would you represent the atom? 7th grade

Gemiola [76]

Answer:

it shows the breakdown of the atom

Explanation:

it will show it molecularly

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3 years ago

Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant at for the following reaction. N2(g)H

soldier1979 [14.2K]

<u>Answer:</u> The equilibrium constant for this reaction is $5.85\times 10^{5}$

<u>Explanation:</u>

The equation used to calculate standard Gibbs free change is of a reaction is:

$\Delta G^o_{rxn}=\sum [n\times \Delta G^o_{(product)}]-\sum [n\times \Delta G^o_{(reactant)}]$

For the given chemical reaction:

$3H_2(g)+N_2(g)\rightarrow 2NH_3(g)$

The equation for the standard Gibbs free change of the above reaction is:

$\Delta G^o_{rxn}=[(2\times \Delta G^o_{(NH_3(g))})]-[(1\times \Delta G^o_{(N_2)})+(3\times \Delta G^o_{(H_2)})]$

We are given:

$\Delta G^o_{(NH_3(g))}=-16.45kJ/mol\\\Delta G^o_{(N_2)}=0kJ/mol\\\Delta G^o_{(H_2)}=0kJ/mol$

Putting values in above equation, we get:

$\Delta G^o_{rxn}=[(2\times (-16.45))]-[(1\times (0))+(3\times (0))]\\\\\Delta G^o_{rxn}=-32.9kJ/mol$

To calculate the equilibrium constant (at 25°C) for given value of Gibbs free energy, we use the relation:

$\Delta G^o=-RT\ln K_{eq}$

where,

$\Delta G^o$ = standard Gibbs free energy = -32.9 kJ/mol = -35900 J/mol (Conversion factor: 1 kJ = 1000 J )

R = Gas constant = 8.314 J/K mol

T = temperature = $25^oC=[273+25]K=298K$

$K_{eq}$ = equilibrium constant at 25°C = ?

Putting values in above equation, we get:

$-32900J/mol=-(8.314J/Kmol)\times 298K\times \ln K_{eq}\\\\K_{eq}=e^{13.279}=5.85\times 10^{5}$

Hence, the equilibrium constant for this reaction is $5.85\times 10^{5}$

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3 years ago

a student proposes the following lewis structure for the azide ion. assign a formal charge to each atom in the student's lewis s

AlexFokin [52]

Lewis structures are diagrams that illustrate the bonding between atoms in a molecule as well as any lone pairs of electrons that may exist. They are also known as Lewis dot formulae, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs). Lewis structures are diagrams that illustrate the bonding between atoms in a molecule as well as any lone pairs of electrons that may exist. They are also known as Lewis dot formulae, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs). A Lewis structure can represent any covalently attached molecule as well as coordination compounds. who proposed it in his 1916 article The Atom and the Molecule.