For the reaction 2 CO ( g ) + O 2 ( g ) ⟶ 2 C O 2 ( g ) ; Δ H = − 560 k J . In a 1 L vessel at 500 K , the initial pressure is 70 a t m , and after the reaction, it becomes 40 a t m at a constant

Question

For the reaction 2 CO ( g ) + O 2 ​ ( g ) ⟶ 2 C O 2 ​ ( g ) ; Δ H = − 560 k J . In a 1 L vessel at 500 K , the initial pressure is 70 a t m , and after the reaction, it becomes 40 a t m at a constant volume of 1 L . The internal energy change of the process will be: (All the above gases represent significant deviation from ideal behavior). ( 1 L a t m = 0.1 k J )

TestHub · Accepted Answer

Δ H = Δ U + Δ ( P V ) At constant volume, Δ H = Δ U + V Δ P . Δ H = Δ U + V × ( P 2 ​ − P 1 ​ ) . − 560 = Δ U + 1 × ( 40 − 70 ) L a t m − 560 = Δ U − 30 ( L a t m ) To convert L atm to kJ, use the conversion factor 1 L a t m ≈ 0.1 k J : − 560 = Δ U − 30 × 0.1 ( k J ) − 560 = Δ U − 3 k J Δ U = − 560 + 3 Δ U = − 557 k J

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