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.

Question

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Answer 1

Question

Chapter 10, Problem 10.70QP

(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

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

The given structure is below.

Chemistry: The Science in Context (Fifth Edition), Chapter 10, Problem 10.70QP

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,

$ln(Pvap,T1Pvap,T2)=ΔHvapR(1T2−1T1)$ (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.

$Vapor pressure(torr)Temperature(K)50373111393230413442433805453$

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).

$ln(805torr442 torr)=ΔHvap8.314 J/mol.K(1433 K−1453 K)ln(1.8213)=ΔHvap8.314 J/mol.K(20196149)KΔHvap=0.60×8.314 J/mol×19614920ΔHvap=48.9 kJ/mol_$

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

(b)

Interpretation Introduction

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

(b)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

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 $48.9 kJ/mol$ as calculated above in part (a).

The room temperature in Kelvin is $296 K$ .

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).

$ln(50 torrPvap,T2)=48.9×103 J/mol8.314 J/mol.K(1296 K−1373 K)ln(50 torrPvap,T2)=5884.41.83×(77110408)50 torrPvap,T2=e−0.826Pvap,T2=0.826 torr_$

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

Conclusion

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

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Answer 2

Question

Chapter 10, Problem 10.70QP

(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

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

The given structure is below.

Chemistry: The Science in Context (Fifth Edition), Chapter 10, Problem 10.70QP

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,

$ln(Pvap,T1Pvap,T2)=ΔHvapR(1T2−1T1)$ (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.

$Vapor pressure(torr)Temperature(K)50373111393230413442433805453$

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).

$ln(805torr442 torr)=ΔHvap8.314 J/mol.K(1433 K−1453 K)ln(1.8213)=ΔHvap8.314 J/mol.K(20196149)KΔHvap=0.60×8.314 J/mol×19614920ΔHvap=48.9 kJ/mol_$

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

(b)

Interpretation Introduction

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

(b)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

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 $48.9 kJ/mol$ as calculated above in part (a).

The room temperature in Kelvin is $296 K$ .

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).

$ln(50 torrPvap,T2)=48.9×103 J/mol8.314 J/mol.K(1296 K−1373 K)ln(50 torrPvap,T2)=5884.41.83×(77110408)50 torrPvap,T2=e−0.826Pvap,T2=0.826 torr_$

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

Conclusion

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

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Answer 3

Question

Chapter 10, Problem 10.70QP

(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

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

The given structure is below.

Chemistry: The Science in Context (Fifth Edition), Chapter 10, Problem 10.70QP

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,

$ln(Pvap,T1Pvap,T2)=ΔHvapR(1T2−1T1)$ (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.

$Vapor pressure(torr)Temperature(K)50373111393230413442433805453$

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).

$ln(805torr442 torr)=ΔHvap8.314 J/mol.K(1433 K−1453 K)ln(1.8213)=ΔHvap8.314 J/mol.K(20196149)KΔHvap=0.60×8.314 J/mol×19614920ΔHvap=48.9 kJ/mol_$

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

(b)

Interpretation Introduction

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

(b)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

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 $48.9 kJ/mol$ as calculated above in part (a).

The room temperature in Kelvin is $296 K$ .

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).

$ln(50 torrPvap,T2)=48.9×103 J/mol8.314 J/mol.K(1296 K−1373 K)ln(50 torrPvap,T2)=5884.41.83×(77110408)50 torrPvap,T2=e−0.826Pvap,T2=0.826 torr_$

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

Conclusion

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

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Answer 4

Question

Chapter 10, Problem 10.70QP

(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

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

The given structure is below.

Chemistry: The Science in Context (Fifth Edition), Chapter 10, Problem 10.70QP

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,

$ln(Pvap,T1Pvap,T2)=ΔHvapR(1T2−1T1)$ (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.

$Vapor pressure(torr)Temperature(K)50373111393230413442433805453$

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).

$ln(805torr442 torr)=ΔHvap8.314 J/mol.K(1433 K−1453 K)ln(1.8213)=ΔHvap8.314 J/mol.K(20196149)KΔHvap=0.60×8.314 J/mol×19614920ΔHvap=48.9 kJ/mol_$

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

(b)

Interpretation Introduction

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

(b)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

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 $48.9 kJ/mol$ as calculated above in part (a).

The room temperature in Kelvin is $296 K$ .

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).

$ln(50 torrPvap,T2)=48.9×103 J/mol8.314 J/mol.K(1296 K−1373 K)ln(50 torrPvap,T2)=5884.41.83×(77110408)50 torrPvap,T2=e−0.826Pvap,T2=0.826 torr_$

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

Conclusion

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

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 10, Problem 10.70QP

(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

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

The given structure is below.

Chemistry: The Science in Context (Fifth Edition), Chapter 10, Problem 10.70QP

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,

$ln(Pvap,T1Pvap,T2)=ΔHvapR(1T2−1T1)$ (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.

$Vapor pressure(torr)Temperature(K)50373111393230413442433805453$

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).

$ln(805torr442 torr)=ΔHvap8.314 J/mol.K(1433 K−1453 K)ln(1.8213)=ΔHvap8.314 J/mol.K(20196149)KΔHvap=0.60×8.314 J/mol×19614920ΔHvap=48.9 kJ/mol_$

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

(b)

Interpretation Introduction

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

(b)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

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 $48.9 kJ/mol$ as calculated above in part (a).

The room temperature in Kelvin is $296 K$ .

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).

$ln(50 torrPvap,T2)=48.9×103 J/mol8.314 J/mol.K(1296 K−1373 K)ln(50 torrPvap,T2)=5884.41.83×(77110408)50 torrPvap,T2=e−0.826Pvap,T2=0.826 torr_$

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

Conclusion

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

Answer 6

Chapter 10, Problem 10.70QP

(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

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

The given structure is below.

Chemistry: The Science in Context (Fifth Edition), Chapter 10, Problem 10.70QP

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,

$ln(Pvap,T1Pvap,T2)=ΔHvapR(1T2−1T1)$ (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.

$Vapor pressure(torr)Temperature(K)50373111393230413442433805453$

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).

$ln(805torr442 torr)=ΔHvap8.314 J/mol.K(1433 K−1453 K)ln(1.8213)=ΔHvap8.314 J/mol.K(20196149)KΔHvap=0.60×8.314 J/mol×19614920ΔHvap=48.9 kJ/mol_$

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

Answer 7

Chapter 10, Problem 10.70QP

(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.

Answer 8

(a)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Explanation

Given

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

The given structure is below.

Chemistry: The Science in Context (Fifth Edition), Chapter 10, Problem 10.70QP

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,

$ln(Pvap,T1Pvap,T2)=ΔHvapR(1T2−1T1)$ (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.

$Vapor pressure(torr)Temperature(K)50373111393230413442433805453$

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).

$ln(805torr442 torr)=ΔHvap8.314 J/mol.K(1433 K−1453 K)ln(1.8213)=ΔHvap8.314 J/mol.K(20196149)KΔHvap=0.60×8.314 J/mol×19614920ΔHvap=48.9 kJ/mol_$

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

Answer 13

(b)

Interpretation Introduction

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

(b)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Explanation of Solution

Explanation

Given

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

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 $48.9 kJ/mol$ as calculated above in part (a).

The room temperature in Kelvin is $296 K$ .

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).

$ln(50 torrPvap,T2)=48.9×103 J/mol8.314 J/mol.K(1296 K−1373 K)ln(50 torrPvap,T2)=5884.41.83×(77110408)50 torrPvap,T2=e−0.826Pvap,T2=0.826 torr_$

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

Conclusion

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

Answer 14

(b)

Interpretation Introduction

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

Answer 15

(b)

Expert Solution

Answer to Problem 10.70QP

Solution

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

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Explanation

Given

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

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 $48.9 kJ/mol$ as calculated above in part (a).

The room temperature in Kelvin is $296 K$ .

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).

$ln(50 torrPvap,T2)=48.9×103 J/mol8.314 J/mol.K(1296 K−1373 K)ln(50 torrPvap,T2)=5884.41.83×(77110408)50 torrPvap,T2=e−0.826Pvap,T2=0.826 torr_$

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

Conclusion

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

Answer 20

Ch. 10.3 - Prob. 1PE Ch. 10.3 - Prob. 2PE Ch. 10.5 - Prob. 3PE Ch. 10.5 - Prob. 4PE Ch. 10.6 - Prob. 5PE Ch. 10.7 - Prob. 6PE Ch. 10.8 - Prob. 7PE Ch. 10 - Prob. 10.1VP Ch. 10 - Prob. 10.2VP Ch. 10 - Prob. 10.3VP

Answer to Problem 10.70QP

Explanation of Solution

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

Answer to Problem 10.70QP

Explanation of Solution

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