In a coffee cup calorimeter 50.0 mL of 0.100 M AgNO3 at 22.6⁰C are mixed with 50.0 mL of 0.100 M HCl, also at 22.6⁰C. The final temperature of the resulting solution is 27.9⁰C. The final solution has a combined mass of 100.0 grams and a specific heat capacity of 4.18 J/g⁰C. a. Write a balanced equation for this reaction. b. Write the net ionic equation for this reaction. c. How many moles of solid product are formed?
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.
In a coffee cup calorimeter 50.0 mL of 0.100 M AgNO3 at 22.6⁰C are mixed with 50.0 mL of 0.100 M HCl, also at 22.6⁰C. The final temperature of the resulting solution is 27.9⁰C. The final solution has a combined mass of 100.0 grams and a specific heat capacity of 4.18 J/g⁰C.
a. Write a balanced equation for this reaction.
b. Write the net ionic equation for this reaction.
c. How many moles of solid product are formed?
d. Calculate the enthalpy change that accompanies this reaction (∆H) in kJ/mole of solid product.
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
