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Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro
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A 1.20 g sample of dry ice is added to a 755 mL flask

Chapter 5, Problem 63E

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QUESTION:

A \(1.20 \mathrm{~g}\) sample of dry ice is added to a \(755 \mathrm{~mL}\) flask containing nitrogen gas at a temperature of \(25.0{ }^{\circ} \mathrm{C}\) and a pressure of \(725 \mathrm{mmHg}\). The dry ice sublimes (converts from solid to gas) and the mixture returns to \(25.0^{\circ} \mathrm{C}\). What is the total pressure in the flask?

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QUESTION:

A \(1.20 \mathrm{~g}\) sample of dry ice is added to a \(755 \mathrm{~mL}\) flask containing nitrogen gas at a temperature of \(25.0{ }^{\circ} \mathrm{C}\) and a pressure of \(725 \mathrm{mmHg}\). The dry ice sublimes (converts from solid to gas) and the mixture returns to \(25.0^{\circ} \mathrm{C}\). What is the total pressure in the flask?

ANSWER:

Problem 63EA 1.20 g sample of dry ice is added to a 755 mL flask containing nitrogen gas at atemperature of 25.0 °C and a pressure of 725 mmHg. The dry ice sublimes (converts fromsolid to gas) and the mixture returns to 25.0 °C. What is the total pressure in the flask Step by step solutionStep 1 of 3From the given,Mass of dry ice sample = 1.20 gVolume = 755 mlDry ice molecular formula =Molar mass of dry ice = 44 g/molLet’s calculate the number of moles of dry ice.Hence, the number of moles of dry ice is 0.0273 mol.

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