Concept explainers
(a)
Interpretation:
The rate of heat removal to produce
Concept introduction:
According to the Hess’s law, the total enthalpy for a reaction is the sum of all the changes in the multiple steps of the reaction. According to this law, enthalpy is a state function.
Specific heat capacity
Here,
Change in specific enthalpy
The rate of heat transfer is calculated as:
(b)
Interpretation:
An expression for the rate of heat removal is to be written in terms of the heat capacities and latent heats of
Concept introduction:
According to the Hess’s law, the total enthalpy for a reaction is the sum of all the changes in the multiple steps of the reaction. According to this law, enthalpy is a state function.
Specific heat capacity
Change in specific enthalpy
The rate of heat transfer is calculated as:
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ELEMENTARY PRINCIPLES OF CHEM. PROCESS.
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- A quantity of ice at 0C is added to 64.3 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C).arrow_forwardThe reaction enthalpy for sublimation of 1 mol solid iodine at 25 C and 1 bar is 62.4 kJ. (Sublimation means changing directly from solid to gas.) I2(s)I2(g)rH=62.4kJ (a) Calculate the heat transfer required to vaporize 10.0 g solid iodine. (b) If 3.42 g iodine vapor changes to solid iodine, calculate the heat transfer. (c) Is the process in part (b) exothermic or endothermic?arrow_forwardSublimation is the phase change from solid to gas without going through a liquid phase. Solid CO2, called dry ice, is an example of one substance that sublimed. Use Hesss law to show that the enthalpy of sublimation, subH, is equal to fusH vapH.arrow_forward
- Calculate the quantity of heating required to convert the water in four ice cubes (60.1 g each) from H2O(s) at 0 °C to H2O(g) at 100. °C. The enthalpy of fusion of ice is 333 J/g and the enthalpy of vaporization of liquid water is 2260 J/g.arrow_forwardChloromethane, CH3CI, arises from microbial fermentation and is found throughout the environment. It is also produced industrially, is used in the manufacture of various chemicals, and has been used as a topical anesthetic. How much energy is required to convert 92.5 g of liquid to a vapor at its boiling point, 24.09 C? (The heat of vaporization of CH3Cl is 21.40 kJ/mol.)arrow_forwardWhich requires the absorption of a greater amount of heat—vaporizing 100.0 g of benzene or boiling 20.0 g of water? (Use Table 8.2.)arrow_forward
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