What is the mass of the solid NH4Cl formed when 73.0 g of NH3(g) are mixed with an equal mass of gaseous HCl? What is the volume and identity of the gas remaining, measured at 14.0°C and 752 mmHg?
What is the mass of the solid NH4Cl formed when 73.0 g of NH3(g) are mixed with an equal mass of gaseous HCl? What is the volume and identity of the gas remaining, measured at 14.0°C and 752 mmHg?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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What is the mass of the solid NH4Cl formed when 73.0 g of NH3(g) are mixed with an equal mass of gaseous HCl? What is the volume and identity of the gas remaining, measured at 14.0°C and 752 mmHg?
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Step 1
Given : The reactants are NH3 and HCl.
Mass of NH3 taken = 73.0 g
Mass of HCl taken 73.0 g
Temperature = 14.0 oC
And pressure = 752 mm Hg = 752 / 760 = 0.9895 atm approx. (since 1 atm = 760 mm Hg)
Molar mass of NH3 = Atomic mass of N + Atomic mass of H X 3 = 14 + 1 X 3 = 17 g/mol.
And molar mass of HCl = Atomic mass of H + Atomic mass of Cl = 1 + 35.5 = 36.5 g/mol.
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