Chemistry problem??

what is the mass of the solid NH4Cl formed when 73.0 g of NH3 are mixed with an equal mass of HCl? what is the volume of the gas remaining, measured at 14.0 degrees celcius and 752 mmHg ? what gas is it?

I need help to set it up. any suggestions?

Answer:
Molecular weight NH3 = 17 g/mol
73.0 / 17 = 4.28 moles NH3
Molecular weight HCl = 36.46 g/mol
73.0 / 36.46 = 2.00
We get 2.00 moles NH4Cl ( MW = 53.45 g/mol ) >>106.9 g
Moles NH3 in excess = 4.28 - 2.00 = 2.28
p = 752 / 760 = 0.989 atm
T = 14 + 273 = 287 K
V = nRT /p = 2.28 x 0.0821 x 287 / 0.989 = 54.3 L

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