Chemistry
Chemistry
4th Edition
ISBN: 9780393919370
Author: Thomas R. Gilbert
Publisher: NORTON
Question
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Chapter 10, Problem 10.64QP

(a)

Interpretation Introduction

Interpretation: The heat of vaporization of the given benzaldehyde. The vapor pressure of the given benzaldehyde at room temperature is to be calculated.

Concept introduction: Vapor pressure is defined as the pressure applied by the molecule in the vapor state is in equilibrium with the solid or liquid state of the same molecule in a closed space.

The factors affect the vapor pressure of a liquid are temperature, surface area and type of a liquid.

If the molecule in the liquid state is more volatile means it will be evaporates easily so it vapors pressure is higher than the other molecule in the liquid state.

To determine: The heat of vaporization of benzaldehyde using the given table.

(a)

Expert Solution
Check Mark

Answer to Problem 10.64QP

Solution

The heat of vaporization of benzaldehyde is 48.9kJ/mol_ .

Explanation of Solution

Explanation

Given

The value of R is 8.314J/mol.K .

The given structure is below.

Chemistry, Chapter 10, Problem 10.64QP

Figure 1

In the above Figure, the structure of benzaldehyde is depicted.

The benzaldehyde is responsible for the aroma of cherries which is depicted in the figure.

The clausius-clapeyron equation states the relation between vapor pressure and the absolute temperature.

The clausius-clapeyron equation is,

ln(Pvap,T1Pvap,T2)=ΔHvapR(1T21T1) (1)

Where,

  • Pvap,T1 is vapor pressure at temperature T1 .
  • Pvap,T2 is vapor pressure at temperature T2 .
  • ΔHvap is heat of vaporization.
  • R is universal gas constant.
  • T1 is the first absolute temperature.
  • T2 is the second absolute temperature.

The table of different values of vapor pressure at different temperature of benzaldehyde is given below.

Vaporpressure(torr)Temperature(K)50373111393230413442433805453

Table 1

The heat of vaporization of benzaldehyde is calculated by the above equation (1).

Substitute the any two values of vapor pressure at the corresponding temperature from the table in the equation (1).

ln(805torr442torr)=ΔHvap8.314J/mol.K(1433K1453K)ln(1.8213)=ΔHvap8.314J/mol.K(20196149)KΔHvap=0.60×8.314J/mol×19614920ΔHvap=48.9kJ/mol_

Therefore, the heat of vaporization of benzaldehyde is 48.9kJ/mol_ .

(b)

Interpretation Introduction

To determine: The vapor pressure of the given benzaldehyde at room temperature.

(b)

Expert Solution
Check Mark

Answer to Problem 10.64QP

Solution

The vapor pressure of the given benzaldehyde at room temperature (23°C) is 0.826torr_ .

Explanation of Solution

Explanation

Given

The value of R is 8.314J/mol.K .

The room temperature is 23°C .

The vapor pressure of benzaldehyde at room temperature (23°C) is calculated by equation (1) given in part (a).

The heat of vaporization of benzaldehyde is 48.9kJ/mol as calculated above in part (a).

The room temperature in Kelvin is 296K .

Substitute the given value of R , room temperature and any value of vapor pressure at the corresponding temperature from the above table given in part (a) in the equation (1).

ln(50torrPvap,T2)=48.9×103J/mol8.314J/mol.K(1296K1373K)ln(50torrPvap,T2)=5884.41.83×(77110408)50torrPvap,T2=e0.826Pvap,T2=0.826torr_

Therefore, the vapor pressure of the given benzaldehyde at room temperature (23°C) is 0.826torr_ .

Conclusion

  1. a) The heat of vaporization of benzaldehyde is 48.9kJ/mol_ .
  2. b) The vapor pressure of the given benzaldehyde at room temperature (23°C) is 0.826torr_ .

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Chapter 10 Solutions

Chemistry

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