You mix 40 mL of 0.30 M HCI with 60 mL of 0.30 M KOH in a perfectly insulated solution calorimeler HCI(aq) + KOH(aq) KCI(aq) + H30() The temperature of both solutions before mixing is 22.50 °C. The temperature of the solution rises to 24.06 °C after mixing. What is the enthalpy change per mole of water produced? The specific heat capacity of water and the solution is 4.2 J/g K. Assume the density of all solutions is 1.00 g/mL. A. 16 kJ B. 840 kJ C. -660 kJ D. 3.6x102 kJ E. -55 kJ amaining
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.
![**Problem Statement:**
You mix 40 mL of 0.30 M HCl with 60 mL of 0.30 M KOH in a perfectly insulated solution calorimeter. The following reaction occurs:
\[ \text{HCl(aq) + KOH(aq) } \rightarrow \text{ KCl(aq) + } H_2O(l) \]
The temperature of both solutions before mixing is \( 22.50 \, ^\circ \text{C} \). The temperature of the solution rises to \( 24.06 \, ^\circ \text{C} \) after mixing. What is the enthalpy change per mole of water produced? The specific heat capacity of water and the solution is \( 4.2 \, \text{J/g·K} \). Assume the density of all solutions is \( 1.00 \, \text{g/mL}. \)
**Options:**
A. \( -16 \, \text{kJ} \)
B. \( -840 \, \text{kJ} \)
C. \( -660 \, \text{kJ} \)
D. \( -3.6 \times 10^2 \, \text{kJ} \)
E. \( -55 \, \text{kJ} \)
**Instructions:**
Select the correct enthalpy change per mole of water produced.
- Click "Submit Answer" to confirm your selection.
- Click "Try Another Version" to attempt a different variation of the question.
1 item attempt remaining.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fec613250-7b04-4f73-98df-322d29ab7281%2Fa95f20ad-db3f-419e-bec1-5a0c743c665a%2Fk3ft3ug_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 2 images
