The manufacture of nitrogen trifluoride is a growing industry, due to its use as a plasma etchant in the semiconductor industry. Nitrogen trifluoride can be synthesized by passing a current through a high-temperature mixture of ammonium fluoride and hydrogen fluoride, with hydrogen gas as a byproduct. In one synthesis, 1.20x103 g ammonium fluoride is reacted with 1.20x103 g hydrogen fluoride to produce 5.00x102 g nitrogen trifluoride. What is the limiting reactant, excess reactant, theoretical yield of nitrogen trifluoride, percent yield, and mass of excess reactant remaining after the reaction?
The manufacture of nitrogen trifluoride is a growing industry, due to its use as a plasma etchant in the semiconductor industry. Nitrogen trifluoride can be synthesized by passing a current through a high-temperature mixture of ammonium fluoride and hydrogen fluoride, with hydrogen gas as a byproduct. In one synthesis, 1.20x103 g ammonium fluoride is reacted with 1.20x103 g hydrogen fluoride to produce 5.00x102 g nitrogen trifluoride. What is the limiting reactant, excess reactant, theoretical yield of nitrogen trifluoride, percent yield, and mass of excess reactant remaining after the reaction?
Given:
Mass of ammonium fluoride = 1.20 x 103 g
Mass of hydrogen fluoride = 1.20 x 103 g
Mass of nitrogen trifluoride = 5.00 x 102 g
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