For the reaction.
`2CO(g)+O_(2)(g)to2CO_(2)(g),DeltaH=-560kJmol^(-1)`
In one litre vessel at 500 K the initial pressure is 70 atm and after the reaction it becomes 40 atm at constant volume of one litre. Calculate change in internal energy. All the above gases show significant deviation from ideal behaviour. (1 L atm = 0.1 kJ)

For the reaction 2CO(g) +O_(2)(g) rarr 2CO_(2)(g) , DeltaH=-560 kJ mol^(-1) In 1 litre vessel at 500 K, the initial pressure is 70 atm and after the reaction, it becomes 40 atm at constant volume of one litre. All the above gases show significant deviation from ideal behavious (1 L atm =0.1 kJ). the change in internal energy will be

For the real gases reaction, 2CO(g)+O_(2)(g)to2CO_(2)(g),DeltaH=-560 kJ. In 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 :

For the real gases reaction 2CO(g)+O_(2)(g)rarr2CO_(2)(g) : DeltaH=-560kJ . In a 10 litre rigid vesel at 500K , the initial pressure is 70 bar and after the reaction it becomes 40 bar. The change in internal energy is:

For the reaction C(s)+CO_(2)(g) rarr 2CO(g) an equilibrium mixture has parital pressure, for CO_(2) and CO, of 4.0 and 8.0 atm respectively . K_(p) for the reaction is

One litre of oxygen at a pressure of 1 atm and two litres of nitrogen at a pressure of 0.5 atm are introduced into a vessel of volume 1 litre. If there is no change in temperature, the final pressure of the mixture of gas (in atm) is