Solution Found!
Answer: The following procedure is a simple though
Chapter 5, Problem 127P(choose chapter or problem)
The following procedure is a simple though somewhat crude way to measure the molar mass of a gas. A liquid of mass 0.0184 g is introduced into a syringe like the one shown here by injection through the rubber tip using a hypodermic needle. The syringe is then transferred to a temperature bath heated to \(45^{\circ} \mathrm{C}\), and the liquid vaporizes. The final volume of the vapor (measured by the outward movement of the plunger) is 5.58 mL and the atmospheric pressure is 760 mmHg. Given that the compound's empirical formula is \(\mathrm{CH}_{2}\), determine the molar mass of the compound.
Questions & Answers
QUESTION:
The following procedure is a simple though somewhat crude way to measure the molar mass of a gas. A liquid of mass 0.0184 g is introduced into a syringe like the one shown here by injection through the rubber tip using a hypodermic needle. The syringe is then transferred to a temperature bath heated to \(45^{\circ} \mathrm{C}\), and the liquid vaporizes. The final volume of the vapor (measured by the outward movement of the plunger) is 5.58 mL and the atmospheric pressure is 760 mmHg. Given that the compound's empirical formula is \(\mathrm{CH}_{2}\), determine the molar mass of the compound.
ANSWER:
Step 1 of 3
Here, we are going to determine the molar mass of the compound.
Calculation of molar mass of the compound.
Given that,
1.0 atm = 760 mm Hg
= 1.0 atm
Mass of the compound = 0.0184 g