Question

Ammonia and gaseous hydrogen chloride combine to form ammonium chloride. NH3+HCL->NH4CL if 4.21 L of NH3(g) at 27 C and 1.02 atm is combined with 5.35 L of HCL(g) at 26 C and 0.998 atm what mass of NH4Cl(s) will be produced? which gas is the limiting reactant? which gas is present in excess

Answer 1

the equation is already balanced (always be sure to check first) so we can move to the stoichiometry

first, let's figure out how many moles of each reactant we have.
convert the temperatures from celcius to kelvin by adding 273.15 to each temperature.

Use PV = nRT (we're in atmospheres, L, moles, and Kelvin, so our constant is R = 0.0821 L⋅atm⋅K^−1⋅mol^−1), plug in the pressure, volume, R, and temperature for each reactant, and calculate how many moles of each reactant you have

from there, you can calculate how many moles of product you will make from 1. the NH3 and 2. the HCl

whichever of those two makes *less* product is the limiting reactant. the other will be in excess.