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photoshop1234 [79]
3 years ago
14

Why were chlorofluorocarbons first developed?

Chemistry
1 answer:
Sergio [31]3 years ago
5 0
CFCs and their associated compounds were developed in the early 1900s as a non-toxic, non-flammable solution to other more dangerous products such as ammonia.
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Which sentence describes an example of sublimation?
Strike441 [17]
<span>An example of sublimation is when a dry ice changes to carbon dioxide when kept in an open container. Sublimation is a change from solid phase to gas phase without passing through the liquid state. In this example, it is clear that the dry ice is solid form and it evaporates as gas without passing through the liquid state.</span>
5 0
3 years ago
HELP PLEASE I HAVE A TEST TODAY AND I DON'T UNDERSTAND ANY OF THIS...
myrzilka [38]

Answer:

About 67 grams or 67.39 grams

Explanation:

First you would have to remember a few things:

 enthalpy to melt ice is called enthalpy of fusion.  this value is 6.02kJ/mol

  of ice  

 it takes 4.18 joules to raise 1 gram of liquid water 1 degree C

 water boils at 100 degrees C and water melts above 0 degrees C

 1 kilojoules is 1000 joules

  water's enthalpy of vaporization (steam) is 40.68 kJ/mol

  a mole of water is 18.02 grams

  we also have to assume the ice is at 0 degrees C

Step 1

Now start with your ice.  The enthalpy of fusion for ice is calculated with this formula:

q = n x ΔH    q= energy, n = moles of water, ΔH=enthalpy of fusion

Calculate how many moles of ice you have:

150g x (1 mol / 18.02 g) = 8.32 moles

Put that into the equation:

q = 8.32 mol x 6.02 = 50.09 kJ of energy to melt 150g of ice

Step 2

To raise 1 gram of water to the boiling point, it would take 4.18 joules times 100 (degrees C)  or 418 joules.

So if it takes 418 joules for just 1 gram of water, it would take 150 times that amount to raise 150g to 100 degrees C.  418 x 150 = 62,700 joules or 62.7 kilojoules.

So far you have already used 50.09 kJ to melt the ice and another 62.7 kJ to bring the water to boiling.  That's a total of 112.79 kJ.

Step 3

The final step is to see how much energy is left to vaporize the water.

Subtract the energy you used so far from what you were told you have.

265 kJ - 112.79 kJ = 152.21 kJ

Again q = mol x ΔH (vaporization)

You know you only have 152.21 kJ left so find out how many moles that will vaporize.

152.21 kJ = mol x 40.68  or   mol = 152.21 / 40.68  = 3.74 moles

This tells you that you have vaporized 3.74 moles with the energy you have left.

Convert that back to grams.

3.74 mol   x  ( 18.02 g / 1 mol ) = 67.39 grams

5 0
2 years ago
If liquid water is exposed to normal atmospheric pressure, what needs to change in order to change its state of matter?
inn [45]

Answer: Option (b) is the correct answer.

Explanation:

State of a substance changes when heat is provided to a substance.

This is because when we heat water then intermoleclar forces present within its molecules tend to break down. Due to this molecules start to move away from each other.

As a result, kinetic energy of molecules increases and they collide rapidly. Hence, solid state of water changes into liquid state and upon excessive heating liquid state of water changes into vapor state.

Thus, we conclude that temperature of water needs to change in order to change its state of matter.

6 0
3 years ago
Read 2 more answers
Using the reaction below determine the amount of Sulfur proceduced in grams (this is a limiting reaction question) 2 H2S + SO2 -
marusya05 [52]

Answer:

<u>= 2.2 g pf S. produced</u>

Explanation:

Balanced Reaction equation:

2H_{2} S + SO_{2} →  3S + 2H_{2} O

1 mole of H2S - 34.1g

? moles - 3.2g

= 3.2/34.1 =<u> 0.09 moles of H2S</u>

Also,

1 mole of S02 - 64.07 g

? moles - 4.42g

= 4.42/64.07 <u>= 0.069 moles of SO2</u>

<u />

<em>Meaning SO2 is the limiting reagent</em>

Finally, 3 moles of S -  32g of sulphur

0.069 mole = ? g of Sulphur

= 0.069 x 32

<u>= 2.2 g pf S.</u>

7 0
2 years ago
How many grams of oxygen are required to burn 0.10mole of c3h8?
Anastaziya [24]
1mol—44g/mol
0.10mol—x
x=0.10*44
x=4.4 g
8 0
3 years ago
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