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(A): At 1200K iron can be reduce cuprous...

(A): At 1200K iron can be reduce cuprous oxide
(R )L: At 1200K, `Fe+Cu_(2)O to FeO+2Cu`
`DeltaG=-300kj//"mole"`

A

If both (A) and (R ) are correct and (R ) is the correct explantion of (A )

B

If both (A) and (R ) are correct and (R ) is not the correct explantion of (A )

C

If (A) is correct but (R ) is incorrect

D

If (A) is incorrect but (R ) is correct

Text Solution

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The correct Answer is:
A
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For the equilibrium: CO_((g))+H_(2)O_((g))hArrCO_(2(g))+H_(2(g)) the standard enthalpy and entropy changes at 300 K and 1200 K for the forward reaction are as follows: {:(DeltaH_(300 K)^(@)=-41.16kJmol^(-1),), (DeltaS_(300 K)^(@)=-0.0424kJmol^(-1)), (DeltaH_(1200 K)^(@)=-32.93kJmol^(-1),), (DeltaS_(1200K)^(@)=-0.0296kJmol^(-1)):} In which direction will the reaction be spontaneous? ( a ) At 300 K , ( b ) At 1200 K , when at equilibrium P_(CO)=P_(CO_(2))=P_(H_(2))=P_(H_(2)O)=1atm Also calculate K_(p) for the reaction at each temperature.