For the reaction CO_((g))+(1)/(2)O_(2(g))rarrCO_(2(g)),DeltaH and DeltaS " are "-283 kJ and -87 JK^(-1).Respectively. It was intended to carry out this reaction at 1000, 1500, 3000 and 3500 K. At which of these temperature would this reaction be thermodynamically spontaneous

For the reaction CO_((g))+(1)/(2)O_(2(g))rarrCO_(2(g)),DeltaH and Delt

1.	For the reaction CO_((g))+(1)/(2)O_(2(g))rarrCO_(2(g)),DeltaH and DeltaS " are "-283 kJ and -87 JK^(-1).Respectively. It was intended to carry out this reaction at 1000, 1500, 3000 and 3500 K. At which of these temperature would this reaction be thermodynamically spontaneous
Answer» 1500 and 3500 K 3000 and 3500 K 1000, 1500 and 3000 K 1500, 3000 and 3500 K Solution :`DELTAG=DeltaH-TDeltaS` For SPONTANEOUS reaction `DeltaG` should be negative When T=1000 K, `DeltaG`=(-283 -1000 `xx` 0.087) kJ =-370 kJ When `T=1500 K, DeltaG=(-283-1500xx0.087) kJ =-413.5 kJ` `T=3000 K, DeltaG=(-283-3000xx0.087) kJ=-544kJ` When `T=3500 K, DeltaG=(-283-3500xx0.087) kJ=+21.5kJ` Hence at 3500 K, reaction will be non-spontaneous.