🤓 Based on our data, we think this question is relevant for Professor Hosseinzadehshahri's class at UB.
Ammonia, NH3(g), and hydrogen chloride, HCl(g), react to form solid ammonium chloride, NH4Cl(s):
NH3(g) + HCl(g) → NH4Cl(s)
Two 2.50 L flasks at 30.0 oC are connected by a stopcock, as shown in the drawing
One flask contains 5.60g NH3(g), and the other contains 4.60 g HCl(g). When the stopcock is opened, the gases react until one is completely consumed.
What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.)
Balanced reaction: NH3(g) + HCl(g) → NH4Cl(s)
Step 1: Calculate the number of moles of each reactant then determine the amount of products produced by each
Molar masses of NH3(g) and HCl(g) will be needed to convert grams to moles