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8 public questions tagged with this topic.

First Law of Thermodynamics Applications

How much heat is required to raise the temperature of 0.3 kg of silver from 35^circ C to 65^circ C ? (Specific heat of s

**First law of thermodynamics** ΔU = Q - W, ΔU internal energy change (J), Q heat added to system (J), W work done by system (J), sign convention physics Q positive when added, W positive when done by system, energy conservation, for isochoric W=0 ΔU=Q, for adiabatic Q=0 ΔU=-W, for isothermal ΔU=0 Q=W, for cyclic ΔU=0 Q_net=W_net. Δ Q = m s Δ T . m = 0.3 , s = 236.1 , Δ T = 65 - 35 = 30 . Δ Q = 0.3 × 236.1 × 30 = 2124.9 J ≈ 2125 J . Using first law ΔU = Q - W,

Ref: NCERT > Physics Book > Thermodynamics > First Law of Thermodynamics Applications

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Adiabatic Processes and Gamma Determination

How much heat is required to raise the temperature of 0.2 kg of silver from 30^circ C to 50^circ C ? (Specific heat of s

**Adiabatic process** no heat exchange Q=0, first law ΔU = -W, for ideal gas P V^γ = constant, T V^{γ-1}= constant, P^{1-γ} T^{γ}= constant, γ = C_p/C_v = (f+2)/f, monatomic γ=5/3, diatomic γ=7/5. Work done W = (P₁V₁ - P₂V₂)/(γ-1), temperature changes due to work. Δ Q = m s Δ T . m = 0.2 , s = 236.1 , Δ T = 50 - 30 = 20 . Δ Q = 0.2 × 236.1 × 20 = 944.4 J ≈ 944 J . Using first law ΔU = Q - W, W = ∫ P dV, isobaric W = P ΔV, isothermal W

Ref: NCERT > Physics Book > Thermodynamics > Adiabatic Processes and Gamma Determination

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