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Which one of the following equations does not correctly represent the first law of thermodynamics for the given process

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a

Isothermal process : q=−w

b

Cyclic process : q=−w

c

Isochoric process : ΔE=q

d

Adiabatic process : ΔE=−w

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detailed solution

Correct option is D

In adiabatic process. 110 heat is allowed to enter or leave the system, i.e. q = 0 Substituting this value in first law of thermodynamics.ΔE=q+W we get ΔE=WIn adiabatic expansion, work is done by the system on the surroundings hence W is negative. Accordingly , ∆E is also negative. i.e. internal energy decreases. In adiabatic compression. W is positive, ∆E is also positive

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For the reaction $C_{2} H_{6} \to C_{2} H_{4} + H_{2}$ the reaction enthalpy $Δ_{l} H = kJ {mol}^{- 1}$ (Round off to the Nearest Integer) [Given : Bond enthalpies in $K J {mol}^{- 1} : C - C = 347, C = C = 611 C - H = 414, H - H = 436]$

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