Reactions – Theoretical and Experimental Yield Help Please?
Author: Mark Jeffries
Question by NNZ1991: Reactions – Theoretical and Experimental Yield Help Please?
How would I go about doing this problem (setup 1st few steps)? An experiment that led to the formation of the new field of organic chemistry involved the synthesis of urea, CN2H4O, by the controlled reaction of ammonia and carbon dioxide.
2 NH3(g) + CO2(g) CN2H4O(s) + H2O(l)
What is the theoretical yield of urea when 100. g of ammonia is reacted with 100. g of carbon dioxide?
I got 56.7g, but that was wrong.
Can someone also check this problem for me.
Magnesium metal, which burns in oxygen with an intensely bright white flame, has been used in photographic flash units. The balanced equation for this reaction is given below.
2 Mg(s) + O2(g) 2 MgO(s)
How many grams of MgO(s) are produced by the complete reaction of 1.41 g of magnesium metal?
Answer I got is 2.34g.
Best answer:
Answer by Ruth N
I checked the second one and you are right.
For the first one, you have to find the limiting reactant( which of the reactants runs out first) which would give you the theoretical yield in the end.
-First you react the 100g of ammonia which gives you 176.47 grams of product
-100g of CO2 gives you 136.36g of product and since this is obviously less(this reactant runs out first), this has to be the theoretical yield also.
-I don’t know if you wanted me to arrange my work so that you could see how i arrived at the amount of product. My guess is that you might have arranged it wrongly somehow.
1. (100) * (1mol/17g of ammonia) * ( 1 mol of urea/2 mol of ammonia) * (60g of ammonia/I mol of ammonia)—>176.47.
2. Same except for 44 instead of 17 and 1/1 mol ratio instead of 1/2 above. This one gives you the 136.36g.
This is all assuming the equation is correct and balanced right.
What do you think? Answer below!
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