1) Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, acc
ID: 823126 • Letter: 1
Question
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 produce 13.87 g of NH3?
b) How many molecules (not moles) of NH3 are produced from 4.47x10^-4 of H2?
2) Hydrobromic acid dissolves solid iron according to the following reaction: Fe (s) + 2HBr (aq) ? FeBr2 (aq) + H2 (g)
a) What mass of H2 would be produced by the complete reaction of the iron bar?
3) ron(III) oxide reacts with carbon monoxide according to the equation:
Fe 2O 3(s)+3CO(g)?2Fe(s)+3CO 2(g)
A reaction mixture initially contains 22.05g Fe2O3and 15.80g CO.
a) once the reaction has occured as completely as possible, what mass (in g) of the excess reactant is left?
4) The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation
3H2(g)+N2(g)?2NH3(g)
The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than 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 reaction under the given conditions?
b) what is the percent yield for this reaction under the given conditions?
Explanation / Answer
1) 3H2(g) + N2(g)?2NH3 (g)
a) Moles of NH3 = 13.87/17 = 0.82
3 moles of H2 peoduces 2 moles of NH3
Thus, moles of H2 required = (3/2) x 0.82 = 1.22
Mass of H2 = 1.22 x 2 = 2.45 gms
b) Moles of H2 = 4.47 x 10^-4/(6.023 x 10^23) = 7.42 x 10^-28
Thus, moles of NH3 formed = (2/3) x 7.42 x 10^-28
molecules of NH3 = (2/3) x 7.42 x 10^-28 x 6.023 x 10^23 = 2.98 x 10^-4
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