What does q with subscript p mean in relation to Constant pressure calorimetry? it seems to mean that if you're in a constant pressure environment, that the calculation of how he flowed, q, is equal to the change in enthalpy. From my reading it also seems to mean that this is only the case and a constant pressure enviriment. if P constant than in a rxn, q = s m change temp = enthalpy of reaction, another term for "heat flow of reaction".
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 does q with subscript p mean in relation to Constant pressure calorimetry?
it seems to mean that if you're in a constant pressure environment, that the calculation of how he flowed, q, is equal to the change in enthalpy. From my reading it also seems to mean that this is only the case and a constant pressure enviriment.
if P constant than in a rxn,
q = s m change temp = enthalpy of reaction, another term for "heat flow of reaction".
![**Thermochemistry**
**What is the mass of the final solution?**
\[ \text{Mass of solution} = 2.00\, \text{L} \times \frac{1000\, \text{mL}}{1\, \text{L}} \times \frac{1.0\, \text{g}}{\text{mL}} = 2.0 \times 10^3 \, \text{g} \]
**What is the temperature increase?**
\[ \Delta T = T_{\text{final}} - T_{\text{initial}} = 28.1^\circ \text{C} - 25.0^\circ \text{C} = 3.1^\circ \text{C} \]
**How much heat is evolved by the reaction?**
\[ \text{Heat evolved} = (4.18\, \text{J/g}^\circ\text{C} \times \text{g})(2.0 \times 10^3\, \text{g})(3.1^\circ \text{C}) = 2.6 \times 10^4\, \text{J} \]
Thus,
\[ q = q_p = \Delta H = -2.6 \times 10^4 \, \text{J} \]
**What is ΔH per mole of BaSO₄ formed?**
Since 1.0 L of 1.0 M Ba(NO₃)₂ contains 1 mole of Ba²⁺ ions and 1.0 L of 1.0 M Na₂SO₄ contains 1.0 mole of SO₄²⁻ ions, 1.0 mole of solid BaSO₄ is formed in the experiment. Thus the enthalpy change per mole of BaSO₄ formed is
\[ \Delta H = -2.6 \times 10^4 \, \text{J/mol} = -26 \, \text{kJ/mol} \]
*See Exercises 6.61 through...*
**Constant-volume calorimetry experiments can also be performed. For example, when a photographic flashbulb flashes, the bulb becomes very hot, because the fine wire of the zirconium or magnesium wire with the oxygen inside the bulb is burned out, and the forming of the white metal oxide occurs inside the bulb, e.g.,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10afd7d2-537b-4ce7-8158-a5546637b29c%2Ff968c037-16fb-42d0-96ec-4e9dd796509b%2Fclkme25.jpeg&w=3840&q=75)
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