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Zanzabum
3 years ago
9

If the volume of an ideal gas is 22.5 L when it is at a temperature of 365 K, what will the volume be when the gas cools to 338K

? Be sure to show your work and proper units.
Chemistry
1 answer:
julsineya [31]3 years ago
6 0

Answer:

20.8L = Final volume of the gas

Explanation:

Based on Charles's law, the volume of a gas is directly proportional to the temperature of the gas under pressure constant. The equation is:

\frac{V_1}{T_1} =\frac{V_2}{T_2}

<em>where V is volume and T absolute temperature of 1, initial state and 2, final state.</em>

<em />

If initial volume is 22.5L, initial T = 365K and final temperature 338K:

22.5L / 365K = V₂ / 338K

<h3>20.8L = Final volume of the gas</h3>
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You have 50 ml of a complex mixture of weak acids that contains some HF (pKa = 3.18) and some HCN (pKa = 9.21). Which is larger,
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\frac{[F^{-}]}{[HF]} is larger

Explanation:

pK_{a}=-logK_{a} , where K_{a} is the acid dissociation constant.

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So, \frac{[F^{-}]}{[HF]} is larger

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What is the temperature of a water body containing a 90% saturation and 11.5 ppm of dissolved oxygen?
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HELP PLEASE I HAVE A TEST TODAY AND I DON'T UNDERSTAND ANY OF THIS...
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Answer:

About 67 grams or 67.39 grams

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First you would have to remember a few things:

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  of ice  

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

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  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.

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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

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