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What is the mass of the solid NH4C1 formed when 73.0 g of
Chapter 5, Problem 59P(choose chapter or problem)
What is the mass of the solid \(\mathrm{NH}_{4} \mathrm{Cl}\) formed when 73.0 g of \(\mathrm{NH}_{3}\) are mixed with an equal mass of HCl? What is the volume of the gas remaining, measured at 14.0°C and 752 mmHg? What gas is it?
Questions & Answers
QUESTION:
What is the mass of the solid \(\mathrm{NH}_{4} \mathrm{Cl}\) formed when 73.0 g of \(\mathrm{NH}_{3}\) are mixed with an equal mass of HCl? What is the volume of the gas remaining, measured at 14.0°C and 752 mmHg? What gas is it?
ANSWER:
Step 1 of 3
The goal of the problem is to find the mass of the solid formed and calculate the volume of the gas remaining, measured at 14.0°C and 752 mmHg and identify the gas.
Given:
Mass of = 73.0 g
T = 14.0°C = 14 + 273 = 287 K
P = 752 mmHg = 0.989 atm.
The balanced equation for the given reaction is: