What mass of NH3 would produce a theoretical yield of 1.00 g of NH4SCN

The balanced chemical equation for the reaction is:

NH3 + HSCN → NH4SCN

From the balanced equation, we can see that one mole of NH3 reacts with one mole of HSCN to produce one mole of NH4SCN.

The molar mass of NH4SCN is approximately 76.12 g/mol. Therefore, 1.00 g of NH4SCN is approximately 0.0131 moles (1.00 g / 76.12 g/mol).

Since the reaction is in a 1:1 ratio, we also need 0.0131 moles of NH3 to produce 1.00 g of NH4SCN.

The molar mass of NH3 is approximately 17.03 g/mol. Therefore, the mass of NH3 needed is approximately 0.223 g (0.0131 moles * 17.03 g/mol).

So, theoretically, 0.223 g of NH3 would produce a yield of 1.00 g of NH4SCN.