3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 12.11°C. Calculate AH for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g•°C and the density of the solution is 1.20 g/mL).
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
3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 12.11°C. Calculate ΔH for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g·°C and the density of the solution is 1.20 g/mL).
### Graphs and Diagrams
The image includes a numeric keypad below the problem statement, likely part of an interactive calculator tool. The keypad features numbers 0-9, a decimal point, a +/- button, and options to clear ("C") and delete ("<x"). It also displays a multiplier button for powers of ten (x 10^□).
### Explanation
To solve the problem, you need to calculate the enthalpy change (ΔH) for the dissolution process using the given data. This involves using the formula for heat change:
\[ q = mc\Delta T \]
- **m** = mass of the solution (in grams)
- **c** = specific heat capacity (J/g·°C)
- **ΔT** = change in temperature (°C)
1. Calculate the mass:
\[ \text{Volume} = 150.0 \, \text{mL} \]
\[ \text{Density} = 1.20 \, \text{g/mL} \]
\[ m = \text{Volume} \times \text{Density} = 150.0 \times 1.20 = 180.0 \, \text{g} \]
2. Substitute into the heat change equation:
\[ q = (180.0 \, \text{g}) \times (4.18 \, \text{J/g·°C}) \times (12.11 \, \text{°C}) = \text{heat absorbed} \]
3. Determine ΔH per mole of solid:
\[ \Delta H = \frac{q}{\text{moles of solid}} \]
Use the numeric keypad to input values and find the precise calculation of ΔH in kJ/mol.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe4f6f55f-74e4-4811-89c3-6145bf7c8bd8%2F22ac4568-6b47-46fd-9ac4-12ff1ee10867%2F00i4hdp_processed.png&w=3840&q=75)
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