Percent yield is 23.11 % when 162.8 g of CO2 are formed from the reaction of excess amount of C8H18 and with 218.0 grams of O2.
Explanation:
Balanced equation for the chemical reaction:
2C8H18 + 25O2 → 16CO2 + 18H2O
data given:
CO2 formed (actual yield) = 162.8 grams
mass of oxygen = 218 grams
16 moles of CO2 formed when 5 moles of oxygen reacted
3.6 moles of CO2 formed when 6.8 moles of oxygen reacted.
In the reaction 16 moles of CO2 will have 44.01 x 16
theoretical yield of CO2 = 704.16 grams
percent yield = x100
putting the values in the above equation
percent yield = x 100
= 0.23 x 100
= 23.11 %
Percent yield is 23.11 %.
They are evnly mixed on the atmotic level but not bonded together.Another nae for a mixture is solution.
Answer:
Explanation:
It is given that pH of .
Now, molality of , M=
Now, we know,
...1
Here C is concentration.
Now,
Putting all values in equation 1.
We get,
Hence, this is the required solution.
The theoretical yield of a reaction is 28% if 25.0 grams of product were actually produced from a reaction that has a 88% yield .
The theoretical yield of a reaction is calculated in following steps .
Identify the limiting reagent, which is the reagent with the fewest moles.
Divide the fewest number of reagent moles by the stoichiometry of the product.
Multiply the result of Step 3 by the molecular weight of the desired product.
theoretical yield : the maximum amount of product that can be produced from a given amount of reactant. this quantity of product is rarely produced during a chemical reaction. limiting reactant.
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