Heat exchanged between the system and surrounding at constant volume is shown by the relation:
Correct answer: B. ∆E= (q)v
- A. ∆H= qv+ w
- B. ∆E= (q)v
- C. ∆H=(q)v
- D. ∆E= (q)v + PV
Explanation
ΔE= q - ΔW ΔE = q - PΔV Where ΔE = change in internal energy q= heat ΔW = work done P = pressure ΔV = volume The equation becomes , q = ΔE + PΔV Let q(v) be the heat absorbed at constant volume thus ΔV = 0 so PΔV also becomes zero Now the equation becomes; ΔE = q(v)
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About Thermochemistry and Energetics of Chemical Reactions
Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
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