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For the reaction Fe2N(s)+(3)/(2)H2(g)=...

For the reaction
`Fe_2N(s)+(3)/(2)H_2(g)=2Fe(s)+NH_3(g)`

A

`K_c=K_p(RT) `

B

`K_c=K_p(RT)^((-1)/(2))`

C

`K_c=K_p(RT)^((1)/(2))`

D

`K_c=K_p(RT)^((3)/(2))`

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For the reaction: Fe_(2)N(s)+(3)/(2)H_(2)(g) hArr 2Fe(s)+NH_(3)(g) (A) K_(c)=K_(p)(RT) (B) K_(c)=K_(p)(RT)^(-1/2) (C) K_(c)=K_(p)(RT)^(1/2) (D) K_(c)=K_(p)(RT)^(3/2)

For the reaction: Fe_(2)N(s)+(3)/(2)H_(2)(g) hArr 2Fe(s)+NH_(3)(g) (A) K_(c)=K_(p)(RT) (B) K_(c)=K_(p)(RT)^(-1/2) (C) K_(c)=K_(p)(RT)^(1/2) (D) K_(c)=K_(p)(RT)^(3/2)

Calculate DeltaH at 85^(@)C for the reaction: Fe_(2)O_(3)(s) +3H_(2)(g) rarr 2Fe(s) +3H_(2)O(l) The data: DeltaH_(298)^(Theta) =- 33.0 kJ mol^(-1) and {:("Substance",Fe_(2)O_(3)(s),Fe(s),H_(2)O(l),H_(2)(g)),(C_(P)^(@)(JK^(-1)mol),103.0,25.0,75.0,28.0):}

Fe_2O_3(s) may be converted to Fe by reaction : Fe_2O_3(s) +3H_2(g)hArr 2Fe(s)+3H_2O(g) For which K_c=8 at temperature 800 K. What percentage of H_2 remains unreacted at equilibrium ?

Fe_(2)O_(3)(s) may be converted to Fe by the reaction Fe_(2)O_(3)(s)+3H_(2)(g)hArr2Fe(s)+3H_(2)O(g) for which K_(c)=8 at temp . 720^(@)c . What percentage of the H_(2) ramains unreacted after the reaction hascome to equilibrium ?

The enthalpy of formation of Fe_(2)O_(3)(s) is -824.2 kJ "mol"^(-1) .Calculate the enthalpy change for the reaction : 4Fe(s) + 3O_(2)(g) to 2Fe_(2)O_(3)(s)

Calculate standard entropy change in the reaction Fe_(2)O_(3)(s)+3H_(2)(g) rarr 2Fe(s)+3H_(2)O(l) Given : S_(m_(0))(Fe_(2)O_(3).S)=87.4,S_(m)^(@)(Fe,S)=27.3 S_(m)^(@)(H_(2),g)=130.7,S_(m)^(@)(H_(2)O,l)=69.9JK^(-1)mol^(-1)

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