This problem is describing a chemical reaction whereby ammonia is produced from nitrogen and hydrogen and asks for the maximum mass of this product when 1.20 g of hydrogen and 11.2 g of nitrogen are reacted. At the end, the answer is d. 6.8 g, considering the following:
In chemistry, chemical equations are used to represent chemical changes in which the reactants get in contact to produce specific products. Thus, the balanced reaction that takes place this time is:
[tex]N_2+3H_2\rightarrow 2NH_3[/tex]
In addition, chemical amounts can be studied via stoichiometry, which is a conversion factor-based methodology for us to convert from the amount of a substance to the amount of another substance whether in grams or moles.
In this case, since we have the mass of the both of the reactants, we calculate the required one with the both of them and then compare:
[tex]1.20g H_2*\frac{1molH_2}{2.02gH_2} *\frac{2molNH_3}{3molH_2}*\frac{17.03gNH_3}{1molNH_3}=6.74gNH_3 \\\\11.2gN_2*\frac{1molN_2}{14.01n_2} *\frac{2molNH_3}{1molN_2}*\frac{17.03gNH_3}{1molNH_3}=27.2gNH_3[/tex]
Whereas the 2:3 and 2:1 are the mole ratios based on the chemical equation. Thus, we see that the hydrogen is the limiting reactant as it produces the smallest result, whereas nitrogen will be in excess, and therefore, the answer is d. 6.8 g.
Learn more about stoichiometry: https://brainly.com/question/9743981
