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3 years ago

Which of the following is the correct molecule for dinitrogen trisulfide?

Chemistry

2 answers:

BabaBlast [244]3 years ago

8 0

Answer:

Option A. N2S3

Explanation:

The easiest way to know this, is to look into the molecules. Let's discart the given options before we choose the correct one.

For beggining we need a moleculae that have 2 atoms of nitrogen and 3 of sulfur.

Option B:

This cannot be the, because for starter, we see the number 2 before the N, this means that is a coefficient and not an atom. An atom of any element is always as subscript. In this molecule, only the number 3 is supposed to be subscripted.

Option C.

We can see that it has only 2 atoms of sulfur, and at the beggining is stated that we need 3, so we can discart rapidly this option.

Option D:

Again, because of the numbers there, we can be confused and think is the correct option, but remember what it was stated before. The atoms should be as subscrip. This is not the case, only the atoms of Nitrogen are subscripted but the number 3 there is put as coefficient, or even can be part of the nitrogen, so instead of being two atoms, we have 23 atoms of Nitrogen.

Therefore, the correct option is A, cause we can see the number 2 and 3 as subscript.

Setler79 [48]3 years ago

4 0

Answer:

A. N2S3

yep u r right

Explanation:

Dinitrogen Trisulfide N2S3 Molecular Weight -- EndMemo.

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The equilibrium constant for the reaction

Hitman42 [59]

The question is incomplete, here is the complete question:

The equilibrium constant for the reaction

N₂O₄(g)⇌2NO₂ at 2°C is Kc = 2.0

If each yellow sphere represents 1 mol of N₂O₄(g) and each gray sphere 1 mol of NO₂ which of the following 1.0 L containers represents the equilibrium mixture at 2°C?

The image is attached below.

Answer: The system which represents the equilibrium having value of $K_c=2.0$ is system (b)

Explanation:

Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_c$

For a general chemical reaction:

$aA+bB\rightarrow cC+dD$

The expression for $K_{c}$ is written as:

$K_{c}=\frac{[C]^c[D]^d}{[A]^a[B]^b}$

For the given chemical equation:

$N_2O_4(g)\rightleftharpoons 2NO_2$

The expression of $K_c$ for above equation follows:

$K_c=\frac{[NO_2]^2}{[N_2O_4]}$ .......(1)

We are given:

Volume of the container = 1.0 L

Value of $K_c$ = 2.0

Molarity of the substance is calculated by using the equation:

$\text{Molarity}=\frac{\text{Number of moles}}{\text{Volume}}$

For the given images:

For a:

Number of Gray spheres = 8 moles

Number of yellow spheres = 4 moles

Putting values in expression 1, we get:

$K_c=\frac{(8/1)^2}{(4/1)}\\\\K_c=16$

For b:

Number of Gray spheres = 4 moles

Number of yellow spheres = 8 moles

Putting values in expression 1, we get:

$K_c=\frac{(4/1)^2}{(8/1)}\\\\K_c=2$

For c:

Number of Gray spheres = 6 moles

Number of yellow spheres = 6 moles

Putting values in expression 1, we get:

$K_c=\frac{(6/1)^2}{(6/1)}\\\\K_c=6$

For d:

Number of Gray spheres = 2 moles

Number of yellow spheres = 8 moles

Putting values in expression 1, we get:

$K_c=\frac{(2/1)^2}{(8/1)}\\\\K_c=\frac{1}{2}$

Hence, the system which represents the equilibrium having value of $K_c=2.0$ is system (b)

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Explanation:

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