4.187/5.°0)(100°C-25°c) b) Calculate the amount of heat involved in the conversion of 25.00 g of water at 100° to steam at 100°. (AH = 40.7 kJ/mol) 25g x 4mole vaporization 1.3872 mn 1. 008
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
What would be the solution to Part B? I'm seeing different methods of solving this, but what would be the most concise means of solving this? Thank you.
![**b) Calculate the amount of heat involved in the conversion of 25.00 g of water at 100°C to steam at 100°C.**
\((\Delta H_{\text{vaporization}} = 40.7 \, \text{kJ/mol})\)
**Solution:**
1. Convert grams to moles:
\[ \frac{25 \, \text{g}}{18.016 \, \text{g/mol}} = 1.3877 \, \text{mol} \]
2. Calculate heat required for vaporization:
\[ q_2 = (1.3877 \, \text{mol}) \times (40700 \, \text{J/mol}) = +56479.4 \, \text{Joules} \]
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**c) Use Hess's law to calculate the amount of heat involved in converting 25.00 g of liquid water at 25°C to steam at 100°C.**
*Note: Some handwritten notes detail sample calculations and conversions, but no diagrams or graphs are present.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F993f9814-1548-4c22-b309-800e507be9a3%2F3bb9ead4-e60e-401b-8d1e-c7835b6ecf79%2Fwpw8ar_processed.jpeg&w=3840&q=75)
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