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Standard XII

Chemistry

Heat Capacity at Constant Pressure

1 mole of an ...

Question

$1$ mole of an ideal non-linear triatomic gas is adiabatically expanded from $16$ atm, $300 K$ to $1$ atm. Calculate $q, W, Δ U, Δ H$ if process is carried out reversibly.

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Solution

Since the process is adiabatic no heat is exchanged between system and surroundings so $q = 0$
$Δ U = q + W$ (eq 1)
$W = - 2.303 n R T l n \frac{P_{1}}{P_{2}}$
Given $P_{1} = 16$ atm
$P_{2} = 1$ atm
$T = 300$ K
$n = 1$
$W = - 2.303 \times 1 \times 8.314 \times 300 l n \frac{16}{1} = - 16084$ J $= - 16.084$ kJ
$Δ U = 16.084$ kJ (From eq 1)

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1 mole of an ideal non-linear triatomic gas is adiabatically expanded from 16 atm, 300K to 1 atm. Calculate q,W,ΔU,ΔH if process is carried out reversibly.

Since the process is adiabatic no heat is exchanged between system and surroundings so q=0ΔU=q+W (eq 1)W=−2.303nRTlnP1P2 Given P1=16 atmP2=1 atmT=300 Kn=1W=−2.303×1×8.314×300ln161=−16084 J=−16.084kJΔU=16.084 kJ (From eq 1)

$1$ mole of an ideal non-linear triatomic gas is adiabatically expanded from $16$ atm, $300 K$ to $1$ atm. Calculate $q, W, Δ U, Δ H$ if process is carried out reversibly.