In a coffee-cup calorimeter, 130.0 mL of 1.0 M NaOH and 130.0 mL of 1.0 M HCl are mixed. Both solutions were originally at 25.7°C. After the reaction, the final temperature is 32.4°C. Assuming that all the solutions have a density of 1.0 g/cm² and a specific heat capacity of 4.18 JCg calculate the enthalpy change for the neutralization of HCI by NaOH Assume that no heat is lost to the surroundings or to the calorimeter. AH-[ kj/mol Submit Answer Try Another Version 1 item attempt remaining
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.
Give typed full explanation not a single word hand written otherwise leave it
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 3 images
