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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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The molar heat of vaporization of carbon disulfide, CS 2 , is 28 . 4 kJ / mol at its normal boiling point of 46  ° C . How much energy (heat) is required to vaporize 1 .0  g of CS 2 at 46  ° C ? How much heat is evolved when 5 0.  g of CS 2 is condensed from the vapor to the liquid form at 46 °C?

Interpretation Introduction

Interpretation:

The heat required to vaporize 1g carbon disulphide and the heat released after condensation of 50g carbon disulphide from vapor to liquid state must be calculated.

Concept Introduction:

During vaporization and condensation there is no temperature change as only latent heat is used for phase change.

Explanation

Heat of vaporization of carbon disulphide is 28.4kJ/mol

So vaporization of 76g carbon disulphide needs 28.4kJ heat energy.

Vaporization of 1g carbon disulphide needs 28.4kJ/76 heat energy =0.374kJ heat energy.

Condensation of 76g carbon disulphide releases 28

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