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masha68 [24]
3 years ago
15

What are possible reasons for a percent yield that is under 100%

Chemistry
1 answer:
matrenka [14]3 years ago
5 0

Answer:

              Percentage Yield is given as,

                 %age Yield  =  Actual Yield / Theoretical Yield × 100

This shows that the %age yield is directly depending upon the actual yield. And most of the time the percentage yield is less than 100 % because of the following factors.

Impure Starting Materials:

                                           If the starting materials (reactants) are not pure then reaction will not completely form the desired product. Different by products will form which will decrease the %age yield.

Incomplete Reactions:

                                     Not all reactions go to completion. In many reactions the starting material after some time stops forming the product due to different conditions. Some reactions attain equilibrium and stop increasing the amount of product. While, in some reactions a by products (like water) formed often react with the product to give a reverse reactions. Hence, the chemistry of reactions also causes the decrease in %age yield.

Handling:

               Another major reason for decrease in yield is handling the product. Always some of the product is lost during the workup of the reaction like, taking TLC, doing solvent extraction, doing column chromatography, taking characterization spectrums. So, we can conclude that the %age yield will always be less than 100%.

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11.7 ml = V

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The air in a bicycle tire is bubbled through water and collected at 25 ∘C. If the total volume of gas collected is 5.30 L at a t
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<u>Answer:</u> The number of moles of gas in bicycle tire is 0.210 moles

<u>Explanation:</u>

To calculate the moles of gas, we use the equation given by ideal gas which follows:

PV=nRT

where,

P = pressure of the gas = 737 torr

V = Volume of the gas = 5.30 L

T = Temperature of the gas = 25^oC=[25+273]K=298K

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Putting values in above equation, we get:

737Torr\times 5.30L=n\times 62.364\text{ L Torr }mol^{-1}K^{-1}\times 298K\\\\n=\frac{737\times 5.30}{62.364\times 298}=0.210mol

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CH3 + HCl &lt;=&gt; CH3Cl + H2O
dmitriy555 [2]

Answer:

The pressure of CH3OH and HCl will decrease.

The final partial pressure of HCl is 0.350038 atm

Explanation:

Step 1: Data given

Kp = 4.7 x 10^3 at 400K

Pressure of CH3OH = 0.250 atm

Pressure of HCl = 0.600 atm

Volume = 10.00 L

Step 2: The balanced equation

CH3OH(g) + HCl(g) <=> CH3Cl(g) + H2O(g)

Step 3: The initial pressure

p(CH3OH) = 0.250atm

p(HCl) = 0.600 atm

p(CH3Cl)= 0 atm

p(H2O) = 0 atm

Step 3: Calculate the pressure at the equilibrium

p(CH3OH) = 0.250 - X atm

p(HCl) = 0.600 - X atm

p(CH3Cl)= X atm

p(H2O) = X atm

Step 4: Calculate Kp

Kp = (pHO * pCH3Cl) / (pCH3* pHCl)

4.7 * 10³ =  X² /(0.250-X)(0.600-X)

X = 0.249962

p(CH3OH) = 0.250 - 0.249962 = 0.000038 atm

p(HCl) = 0.600 - 0.249962 = 0.350038 atm

p(CH3Cl)= 0.249962 atm

p(H2O) = 0.249962 atm

Kp = (0.249962 * 0.249962) / (0.000038 * 0.350038)

Kp = 4.7 *10³

The pressure of CH3OH and HCl will decrease.

The final partial pressure of HCl is 0.350038 atm

4 0
3 years ago
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