CHEMISTRY HIGH SCHOOL

In the pie chart below, which of the following represents the amount of Earth's water located in the oceans?A pie chart with part A representing 2%, part B representing .8%, part C representing .2% and part D representing 97%.


A only
A and B
C only
D only

Answers

Answer 1
Answer: In the pie chart above, the pie chart that represents the amount of Earth's water located in the oceans is D only. The rest of the choices are too small for the amount of water that is present on Earth.
Answer 2
Answer:

Answer: D only.

Explanation:

The amount of Earth's water located in oceans is 97%. Rest 3% is in the form of rivers, glaciers, polar ice-caps, lakes and ground water. Out of this 3% also, only 0.3% is freshwater which found in swamps, lakes and rivers.

In the pie chart, part D represents 97%. Thus, part D only represents the amount of Earth's water located in the oceans.

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Consider the solutions, 0.04 m urea [(NH2)2C=O)], 0.04 m AgNO3 and 0.04 m CaCl2. Which has (i) the highest osmotic pressure, (ii) the lowest vapor pressure, (iii) the highest boiling point?

Answers

Answer:

i) Highest osmotic pressure: CaCl2

ii) lower vapor pressure : CaCl2

iii) highest boiling point : CaCl2

Explanation:

The colligative properties depend upon the number of solute particles in a solution.

The following four are the colligative properties:

a) osmotic pressure : more the concentration of the solute, more the osmotic pressure

b) vapor pressure: more the concentration of the solute, lesser the vapor pressure.

c) elevation in boiling point: more the concentration of the solute, more the boiling point.

d) depression in freezing point: more the concentration of the solute, lesser the freezing point.

the number of particle produced by urea = 1

the number of particle produced by AgNO3 = 2

the number of particle produced by CaCl2 = 3

As concentrations are same, CaCl2 will have more number of solute particles and urea will have least

i) Highest osmotic pressure: CaCl2

ii) lower vapor pressure : CaCl2

iii) highest boiling point : CaCl2

Final answer:

The solution with the highest number of particles in solution (CaCl2 in this case), experiences the highest osmotic pressure, lowest vapor pressure and highest boiling point due to the principles of colligative properties.

Explanation:

The question pertains to the colligative properties of solutions, which would be governed by the number of particles in the solution. The solutions are 0.04 m urea [(NH2)2C=O)], 0.04 m AgNO3, and 0.04 m CaCl2. For (i) Highest osmotic pressure, the solution with the highest ion count would yield the highest osmotic pressure. CaCl2 dissociates into three ions (Ca²+, and 2 Cl¯), therefore, it would exhibit the highest osmotic pressure. For (ii) Lowest vapor pressure, this would coincide with the solution with the highest osmotic pressure, again making it CaCl2, due to the greatest decrease in vapor pressure. For (iii) the highest boiling point, this too would be CaCl2 for the reasons stated above. The presence of more particles in a solution interferes more with the evaporation process, requiring more energy (higher temperature) to achieve boiling.

Learn more about Colligative Properties here:

brainly.com/question/34190054

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Answers

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B. Ionic solids have higher melting points than molecular solids.
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Answers

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Answers

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If 0.25 mol of Br2 and 0.55mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentration of BrCl ?? Br2(g)+Cl2(g) 2BrCl at 400 K, Kc= 7.0

Answers

Answer:

[BrCl] = 0,13M

Explanation:

For the reaction:

Br₂(g) + Cl₂(g) ⇄ 2BrCl

kc = [BrCl]²/[Br₂] [Cl₂] (1)

If initial [Br₂] and [Cl₂] are 0,25mol/3,0L=0,083M and 0,55mol/3,0L=0,18M, the concentrations in equilibrium are:

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[Cl₂] = 0,18M - x

[BrCl] = 2x

Replacing in (1)

7 = (2x)²/ (0,083 - x)(0,18 - x)

7 = 4x²/ x²- 0,263x + 0,01494

7x² - 1,841x + 0,10458 = 4x²

3x² - 1,841x + 0,10458 = 0

Solving for x:

x = 0,0633. As [BrCl] = 2x. [BrCl] = 0,13M

I hope it helps!

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Answers

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