For the real gases reaction 2CO(g) + O2(g)→ 2C O2(g); Δ H = - 560 kJ. In a 10 litre rigid vessel at 500 K, the initial pressure is 70 bar and after the reaction it becomes 40 bar. The change in internal energy is:

Question

For the real gases reaction 2CO(g) + O2(g)→ 2C O2(g); Δ H = - 560 kJ. In a 10 litre rigid vessel at 500 K, the initial pressure is 70 bar and after the reaction it becomes 40 bar. The change in internal energy is: (A) - 557 kJ (B) - 530 kJ (C) - 563 kJ (D) None of these

Tardigrade Admin · Accepted Answer

At constant volumeΔ H=Δ U+VΔ P -560= Δ U+10 ×(-30)×0.1Δ U=-530kJ

Q. For the real gases reaction $2 CO (g) + O_{2} (g) \to 2 C O_{2} (g);$
$Δ H = - 560 k J .$ In a $10$ litre rigid vessel at $500 K,$ the initial pressure is $70$ bar and after the reaction it becomes $40$ bar. The change in internal energy is:

$- 557 k J$

$- 530 k J$

$- 563 k J$

None of these

At constant volume $Δ H = Δ U + V Δ P$
$- 560 = Δ U + 10 \times (- 30) \times 0.1Δ U = - 530 k J$

Q. For the real gases reaction 2CO(g)+O2​(g)→2CO2​(g); ΔH=−560kJ. In a 10 litre rigid vessel at 500K, the initial pressure is 70 bar and after the reaction it becomes 40 bar. The change in internal energy is:

−557kJ

−530kJ

−563kJ