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3H2(g)+N2(g)?2NH3(g)


1.02g H2 is allowed to react with 10.3g N2, producing 1.23g NH3.


What is the theoretical yield for this reaction under the given conditions?


What is the percent yield for this reaction under the given conditions?

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Hubert Koch
Hubert KochLv2
29 Sep 2019

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Related questions

1) Hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas, NH3, according to the equation 3H2(g) +N2(g)?2NH3(g)

a) How many grams of H2 are needed to produce13.87 g of NH3?

b) How many molecules (not moles) of NH3 areproduced from 4.47x10^-4 of H2?


2) Hydrobromic acid dissolves solid ironaccording to the following reaction: Fe (s) + 2HBr (aq)? FeBr2 (aq) + H2 (g)

a) What mass of H2 would be produced by thecomplete reaction of the iron bar?


3) ron(III) oxidereacts with carbon monoxide according to the equation:

Fe 2O3(s)+3CO(g)?2Fe(s)+3CO 2(g)
A reaction mixture initially contains22.05gFe2O3and 15.80gCO.

a) once the reaction has occured as completelyas possible, what mass (in g) of the excess reactant isleft?


4) The Haber-Boschprocess is a very important industrial process. In the Haber-Boschprocess, hydrogen gas reacts with nitrogen gas to produce ammoniaaccording to the equation

3H2(g)+N2(g)?2NH3(g)

The ammonia produced in the Haber-Bosch process hasa wide range of uses, from fertilizer to pharmaceuticals. However,the production of ammonia is difficult, resulting in lower yieldsthan those predicted from the chemical equation.

1.30g H2 is allowed to react with 10.3g N2,producing 2,66 gNH3

a) what is the theoretical yiel for this reactionunder the given conditions?

b) what is the percent yield for this reaction underthe given conditions?

1) Hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas, NH3, according to the equation 3H2(g) +N2(g)?2NH3(g)

a) How many grams of H2 are needed to produce13.87 g of NH3?

b) How many molecules (not moles) of NH3 areproduced from 4.47x10^-4 of H2?


2) Hydrobromic acid dissolves solid ironaccording to the following reaction: Fe (s) + 2HBr (aq)? FeBr2 (aq) + H2 (g)

a) What mass of H2 would be produced by thecomplete reaction of the iron bar?


3) ron(III) oxidereacts with carbon monoxide according to the equation:

Fe 2O3(s)+3CO(g)?2Fe(s)+3CO 2(g)
A reaction mixture initially contains22.05gFe2O3and 15.80gCO.

a) once the reaction has occured as completelyas possible, what mass (in g) of the excess reactant isleft?


4) The Haber-Boschprocess is a very important industrial process. In the Haber-Boschprocess, hydrogen gas reacts with nitrogen gas to produce ammoniaaccording to the equation

3H2(g)+N2(g)?2NH3(g)

The ammonia produced in the Haber-Bosch process hasa wide range of uses, from fertilizer to pharmaceuticals. However,the production of ammonia is difficult, resulting in lower yieldsthan those predicted from the chemical equation.

1.30g H2 is allowed to react with 10.3g N2,producing 2,66 gNH3

a) what is the theoretical yiel for this reactionunder the given conditions?

b) what is the percent yield for this reaction underthe given conditions?

1.91 g H2 is allowed to react with 9.86 g N2, producing 1.74 g NH3. What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units.

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