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Tems11 [23]
3 years ago
8

If more solute can be dissolved in a solvent, the solution is

Chemistry
1 answer:
WARRIOR [948]3 years ago
7 0

Answer:

the answer is unsaturated

Explanation:

A saturated solution contains more solute per volume of solvent than an unsaturated solution. The solute has dissolved until no more can, leaving undissolved matter in the solution. ... In a supersaturated solution, there is more dissolved solute than in a saturated solution.

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The Electron Configuration for Sulfur(S)= 1s^2  2s^2  2p^6  3s^2  3p^4

Explanation:

Use the sheet attached to help with a future question. (Hint: Follow the red lines). The atomic number will be equal to the number of powers raised.

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An aqueous solution has a hydroxide-ion concentration of 1.0 x 10-3 M. What is the pH of the solution?
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Warm air above large bodies of water rises into the atmosphere, carrying with it water vapor that forms clouds. Likewise, as air
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5 0
2 years ago
Tetrahydrofuran (THF) is a common organic solvent with a boiling point of 339 K. Calculate the total energy (q) required to conv
poizon [28]

Explanation:

For the given reaction, the temperature of liquid will rise from 298 K to 339 K. Hence, heat energy required will be calculated as follows.

             Q_{1} = mC_{1} \Delta T_{1}

Putting the given values into the above equation as follows.

           Q_{1} = mC_{1} \Delta T_{1}

                      = 27.3 g \times 1.70 J/g K \times 41

                      = 1902.81 J

Now, conversion of liquid to vapor at the boiling point (339 K) is calculated as follows.

           Q_{2} = energy required = mL_{v}

    L_{v} = latent heat of vaporization

Therefor, calculate the value of energy required as follows.

             Q_{2} = mL_{v}

                         = 27.3 \times 444

                         = 12121.2 J

Therefore, rise in temperature of vapor from 339 K to 373 K is calculated as follows.

            Q_{3} = mC_{2} \Delta T_{2}

Value of C_{2} = 1.06 J/g,    \Delta T_{2} = (373 -339) K = 34 K

Hence, putting the given values into the above formula as follows.

             Q_{3} = mC_{2} \Delta T_{2}

                       = 27.3 g \times 1.06 J/g \times 34 K

                       = 983.892 J

Therefore, net heat required will be calculated as follows.

            Q = Q_{1} + Q_{2} + Q_{3}

                = 1902.81 J + 12121.2 J + 983.892 J

                = 15007.902 J

Thus, we can conclude that total energy (q) required to convert 27.3 g of THF at 298 K to a vapor at 373 K is 15007.902 J.

5 0
3 years ago
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