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Otrada [13]
3 years ago
14

Which material is typically used as a thermal insulator

Chemistry
2 answers:
sp2606 [1]3 years ago
6 0

Answer:

Lots of items.

Explanation:

Fiber, mineral wool, and corks.

Citrus2011 [14]3 years ago
5 0

Answer: plastic, wood, rubber

Explanation:

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Identify the arrows that represent the process of cooling.<br> liquid<br> gas<br> solid
krok68 [10]

The arrows B, C, and E represent the process of cooling.

Solid state: In the solid state, the molecules are arranged in a regular and fixed pattern. The molecules in a solid are closely packed that is the solid particles can not move.

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Gaseous state: In the gaseous state, the molecules are present in an irregular manner. The molecules of gases are not closely packed and can move freely.

Therefore, the solid changes to liquid on heating, and the liquid changes to solid after cooling.

Liquid changes to a gaseous state on heating while gases changes to liquid on cooling.

Solid changes to gas on heating and gases change to solid after cooling.

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6 0
1 year ago
How do you balance nuclear equations?
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The sum of the mass numbers and the sum of the atomic numbers balance on either side of an equation
6 0
3 years ago
Both the freezing temperature and the melting temperature of water are the same(0°C). Explain why a substance like water freezes
Ahat [919]
It is approximately 0. It could be barley higher or lower for both. You have to take the altitude into consideration. 
5 0
3 years ago
If 500.0 mL of 0.10 M Ca2+ is mixed with 500.0 mL of 0.10 M SO42−, what mass of calcium sulfate will precipitate? Ksp for CaSO4
statuscvo [17]

Answer:

The mass of calcium sulfate that will precipitate is 6.14 grams

Explanation:

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

500.0 mL of 0.10 M Ca^2+ is mixed with 500.0 mL of 0.10 M SO4^2−

Ksp for CaSO4 is 2.40*10^−5

<u>Step 2:</u> Calculate moles of Ca^2+

Moles of Ca^2+ = Molarity Ca^2+ * volume

Moles of Ca^2+ = 0.10 * 0.500 L

Moles Ca^2+ = 0.05 moles

<u>Step 3: </u>Calculate moles of SO4^2-

Moles of SO4^2- = 0.10 * 0.500 L

Moles SO4^2- = 0.05 moles

<u>Step 4: </u>Calculate total volume

500.0 mL + 500.0 mL = 1000 mL = 1L

<u>Step 5: </u> Calculate Q

Q = [Ca2+] [SO42-]  

[Ca2+]= 0.050 M   [O42-]

Qsp = (0.050)(0.050 )=0.0025 >> Ksp

This means precipitation will occur

<u> Step 6:</u> Calculate molar solubility

Ksp = 2.40 * 10^-5 = [Ca2+][SO42-] =(x)(x)

2.40 * 10^-5 = x²

x = √(2.40 * 10^-5)

x = 0.0049 M = Molar solubility

<u> Step 7:</u> Calculate total CaSO4 dissolved

total CaSO4 dissolved = 0.0049 M * 1 L * 136.14 mol/L = 0.667 g

<u>Step 8:</u> Calculate initial mass of CaSO4

Since initial moles CaSo4 = 0.050

Initial mass of CaSO4 = 0.050 * 136.14 g/mol

Initial mass of CaSO4 = 6.807 grams

<u>Step 9:</u> Calculate mass precipitate

6.807 - 0.667 = 6.14 grams

The mass of calcium sulfate that will precipitate is 6.14 grams

5 0
3 years ago
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