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mina [271]
2 years ago
6

Suppose that X represents an arbitrary cation and that Y represents an anionic species. Using the charges indicated in the super

script of X and Y, fill in the remaining blanks below by writing the appropriate subscript for each X and Y to balance the net charge on the ionic XaYb compound formed (where a and b represent positive, whole numbers of X and Y, respectively).
Y- Y2- Y3-
X+
X2+ XY2
X3+
Chemistry
1 answer:
dmitriy555 [2]2 years ago
8 0

Answer:

See explanation.

Explanation:

Hello!

In this case, when having the cationic and anionic species with the specified charges, in order to abide by the net charge rule, we need to exchange the charges in the form of subscripts and without the sign, just as shown below:X^{m+}Y^{n-}\rightarrow X_nY_m

Thus, for all the given combinations, we obtain:

- Y⁻

X^+Y^-\rightarrow XY\\\\X^{2+}Y^-\rightarrow XY_2\\\\X^{3+}Y^-\rightarrow XY_3

- Y²⁻

X^+Y^{2-}\rightarrow X_2Y\\\\X^{2+}Y^{2-}\rightarrow X_2Y_2\rightarrow XY\\\\X^{3+}Y^{2-}\rightarrow X_2Y_3

- Y³⁻

X^+Y^{3-}\rightarrow X_3Y\\\\X^{2+}Y^{3-}\rightarrow X_3Y_2 \\\\X^{3+}Y^{3-}\rightarrow X_3Y_3\rightarrow XY

Best regards!

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Where is a divergent boundary most likely to be found?
nexus9112 [7]

Answer:

a

Explanation

Bc I took the test, good luck with that guys

7 0
2 years ago
30. The density of an unknown gas at 27°C and 2 atm pressure is equal with density of N2 gas at
Zanzabum

Answer:

Molar mass of the unknown gas is 64.6 g/mol

Explanation:

Let's think this excersise with the Ideal Gases Law.

We start from the N₂. At STP conditions we know that 1 mol of anything occupies 22.4L.

We apply: P . V = n . R . T

5 atm . V = 1 mol . 0.082 . 325K

V = (1 mol . 0.082 . 325K) / 5 atm = 5.33 L

It is reasonable to say that, if we have more pressure, we may have less volume.

As this is the volume for 1 mol of N₂, our mass is 28 g. Then, the density of the nitrogen and the unknown gas is 28 g/5.33L = 5.25 g/L

Our unknown gas has, this density at 27°C and 2 atm.

If we star from this, again: 1 mol of any gas occupy 22.4L at STP, we can calculate the volume for 1 mol at those conditions:

P₁ . V₁ / T₁ = P₂ . V₂ / T₂

1 atm . 22,4L / 273K = 2 atm . V₂ / 300K

Remember that the value for T° is Absolute (T°C + 273)

[ (1 atm . 22.4L / 273K) . 300K] / 2 atm = V₂ → 12.3L

This is the volume for 1 mol of the unknown gas at 2 atm and 27°C

We use density to determine the mass: 12.3 L . 5.25 g/L = 64.6 g

That's the molar mass: 64.6 g/mol

6 0
2 years ago
Measurements show that unknown compound has the following composition: element mass 38.7 % calcium, 19.9 % phosphorus and 41.2 %
Mademuasel [1]

Answer:

D) empirical formula is: C₃P₂O₈

Explanation:

Given:

Mass % Calcium (Ca) = 38.7%

Mass % Phosphorus (P) = 19.9%

Mass % oxygen (O) = 41.2 %

This implies that for a 100 g sample of the unknown compound:

Mass Ca = 38.7 g

Mass P = 19.9 g

Mass O = 41.2 g

Step 1: Calculate the moles of Ca, P, O

Atomic mass Ca = 40.08 g/mol

Atomic mass P = 30.97 g/mol

Atomic mass O = 16.00 g/mol

Moles\ Ca = \frac{38.7g}{40.08g/mol} =0.966\ mol\\\\Moles\ P = \frac{19.9g}{30.97g/mol} =0.643\ mol\\\\Moles\ O = \frac{41.2g}{16.00g/mol} =2.58\ mol

Step 2: Calculate the molar ratio

C = \frac{0.966}{0.643} =1.50\\\\P = \frac{0.643}{0.643} = 1.00\\\\O = \frac{2.58}{0.643} =4.00

Step 3: Calculate the closest whole number ratio

C: P: O = 1.50 : 1.00 : 4.00

C : P : O = 3:2:8

Therefore, the empirical formula is: C₃P₂O₈

7 0
3 years ago
A 1.044 g sample contains only vitamin C (C6H8O6) and sucralose (C12H19Cl3O8). When the sample is dissolved in water to a total
Strike441 [17]

Answer:

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3 years ago
Read 2 more answers
Why is the vapor pressure of a warm pale higher than the vapor pressure of a cold lake
levacccp [35]

The vapor pressure of a warm pale higher than the vapor pressure of a cold lake because Warm water evaporates more quickly.

Hence, Option B is correct answer.

<h3>What is Evaporation ? </h3>

The process in which a liquid or solid is converted into vapour is called Evaporation. When water gains the heat energy then it changes in to gas. When the temperature increases it speeds up the rate of evaporation.

The temperature of warm water increases, the kinetic energy of the warm water molecule also increases.

Thus from the above conclusion we can say that The vapour pressure of a warm lake is higher than the vapor pressure of a cold lake because Warm water evaporates more quickly.

Hence, Option B is correct answer.

Learn more about the Evaporation here: brainly.com/question/9339710

#SPJ1

Disclaimer: The question was given incomplete on the portal. Here is the complete questions.

Question: Why is the vapor pressure of a warm lake higher than the vapor pressure of a cold lake?

A. Warm water has a greater heat of vaporization.

B. Warm water evaporates more quickly.

C. Cool water evaporates more quickly.

D. Cool water has a greater heat of vaporization.

3 0
1 year ago
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