Chemical Thermodynamics — Flashcards
Maharashtra Board · Class 12 · Chemistry
25 flashcards for Chemical Thermodynamics (Maharashtra Board Class 12 Chemistry) to test yourself on key terms and facts.
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What is a thermodynamic system? Give an example from daily life.
Answer
A thermodynamic system is the part of the universe under study for energy changes. It is separated from the surroundings by boundaries. Example: Hot coffee in a cup - the coffee is the system, while t…
Distinguish between open, closed, and isolated systems with examples.
Answer
Open system: Exchanges both energy and matter (hot coffee in open cup). Closed system: Exchanges only energy, not matter (coffee in covered cup). Isolated system: No exchange of energy or matter (coff…
What are state functions? Give three examples and explain why they are state functions.
Answer
State functions are properties that depend only on the state of the system, not the path taken to reach that state. Examples: Pressure (P), Volume (V), Temperature (T), Internal Energy (U), Enthalpy (…
Write the expression for pressure-volume work and explain the sign convention.
Answer
W = -Pₑₓₜ ΔV = -Pₑₓₜ(V₂ - V₁) Sign convention: +W: Work done ON the system (compression) -W: Work done BY the system (expansion) For expansion: V₂ > V₁, so W is negative For compression: V₂ < V₁, so…
State the First Law of Thermodynamics and write its mathematical expression.
Answer
First Law of Thermodynamics: Energy can neither be created nor destroyed, only converted from one form to another. The total energy of the universe remains constant. Mathematical expression: ΔU = Q +…
Define enthalpy and derive the relationship ΔH = ΔU + PΔV.
Answer
Enthalpy (H) is the sum of internal energy and pressure-volume work: H = U + PV Derivation: ΔH = H₂ - H₁ = (U₂ + P₂V₂) - (U₁ + P₁V₁) ΔH = ΔU + Δ(PV) At constant pressure: P₁ = P₂ = P ΔH = ΔU + PΔV E…
For gas phase reactions, derive ΔH = ΔU + ΔnₘRT.
Answer
Starting from ΔH = ΔU + PΔV For ideal gases: PV = nRT For reactants: PV₁ = n₁RT For products: PV₂ = n₂RT Therefore: PΔV = P(V₂ - V₁) = PV₂ - PV₁ = n₂RT - n₁RT = (n₂ - n₁)RT ΔH = ΔU + ΔnₘRT where Δnₘ…
What is standard enthalpy of formation? Give the thermochemical equation for formation of H₂O(l).
Answer
Standard enthalpy of formation (Δf H°) is the enthalpy change when 1 mole of a compound is formed from its constituent elements in their standard states at 1 bar pressure and 298 K. H₂(g) + ½O₂(g) → …
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