A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5°C) to vapor at 59.0°C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate Δ H for: Br 2 ( l , 22.5 ° C ) → Br 2 ( l , 59.0 ° C ) (b) Calculate Δ H for: Br 2 ( l , 59.0 ° C ) → Br 2 ( g , 59.0 ° C ) (c) Using Hess's law, calculate ΔH for: Br 2 ( l , 22.5 ° C ) → Br 2 ( g , 59.0 ° C )
A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5°C) to vapor at 59.0°C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate Δ H for: Br 2 ( l , 22.5 ° C ) → Br 2 ( l , 59.0 ° C ) (b) Calculate Δ H for: Br 2 ( l , 59.0 ° C ) → Br 2 ( g , 59.0 ° C ) (c) Using Hess's law, calculate ΔH for: Br 2 ( l , 22.5 ° C ) → Br 2 ( g , 59.0 ° C )
Solution Summary: The author explains that the enthalpy change, H, for a reaction is essentially the heat flow of the reaction taking place at constant pressure.
A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5°C) to vapor at 59.0°C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed.
(a) Calculate ΔH for:
Br
2
(
l
,
22.5
°
C
)
→
Br
2
(
l
,
59.0
°
C
)
(b) Calculate ΔH for:
Br
2
(
l
,
59.0
°
C
)
→
Br
2
(
g
,
59.0
°
C
)
(c) Using Hess's law, calculate ΔH for:
Br
2
(
l
,
22.5
°
C
)
→
Br
2
(
g
,
59.0
°
C
)
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Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY