##### chemistry question on limiting reagents

 Chemistry Tutor: None Selected Time limit: 1 Day

153 grams of ammonia and 325 grams of oxygen were reacted according to the following equation:

4NH3 + 5O2 --> 4NO + 6H2O

a) what is the limiting reagent?

b) how many grams of each are produced?

c) what is the percent yield assuming that 204 grams of water were actually produced?

d) compare the total masses of reactant to the total mass of products. what law does this prove?

Apr 26th, 2015

4NH3     +   5O2  ------        4NO         +    6 H2O

9.0 mol     10.16 mol         8.13 mol           12.19 mol

a)  4 moles of NH3 react with 5 moles of O2 hens

9.0 moles of NH3 required 5/4*9 moles of O2 = 11.25 moles of O2 is required

But there are 10.16 moles of O2 is present in reaction flask  hence

Limiting reagent will be O2

B) NO = 8.13 x 30 = 243.9 g , H2O = 12.19 x 18 = 219.46 g

C) % yield = 100 x 204/ 219.6 = 92.89 %

D) Mas of reactant(478g)  , mass of product( 243.9+219.46 = 463.36)

There should be mass of reactant = mass of product by law of conservation of mass

but NH3 is not reacting completely  so  it is not follow this law.

Apr 28th, 2015

Apr 28th, 2015

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Apr 26th, 2015
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Apr 26th, 2015
Dec 4th, 2016
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