Answer:
False
Explanation:
using the measurements of the amounts of chemicals, it can be calculated to some degree of accuracy depending mainly on the accuracy of the measurements and enviroments of the reaction
To predict the theoretical yield we would have to know the amount we of product we actually produced in a reaction, and the amount that should have been produced based on calculations involving the balanced equation for the reaction.
For instance, suppose we made water from hydrogen and oxygen. Starting with 2 moles of hydrogen and 1 mole of oxygen we should produce 2 moles of water (or 36 gram). But suppose we actually ran the reaction in the lab and collected only 34g of water.
The percent yield would be 34g / 36g x 100 =94.4%
So, if I'm reading your question correctly, 20g is the experimental yield and 10% is the percent yield.
Plugging in gives us 10/100 = 20/x
The theoretical yield must be 200g.
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I HOPE THAT HELP MY FRIEND :)
4 mole NH3 forms 6 moles of water, so 2 mole NH3 will form 3 moles of water
<span>The intermolecular forces of attraction between CH3CH2NH2 are dispersion forces and hydrogen bonds. Dispersion forces are due to the ethyl ends of the molecule and the hydrogen bonds are due to the presence of the amine end of the molecule.</span>
