For the reaction of steam on red hot iron: 3 Fe ( s ) + 4 H ₂ O ( g ) Fe ₃ O ₄( s ) + 4 H ₂( g ) The value of K_c is 2.5 at 1000 ~K . What will be the value of K_p for this reaction at the same temperature? (Given: R = 0.083 ~L~bar~K ⁻¹ mol ⁻¹ )

Step-by-step solution

For the given heterogeneous reaction: 3 Fe ( s ) + 4 H ₂ O ( g ) Fe ₃ O ₄( s ) + 4 H ₂( g ) The change in the number of moles of gaseous species ( n_g ) is calculated by considering only the gaseous products and reactants, strictly ignoring the solid species. n_g = moles of H ₂( g ) - moles of H ₂ O ( g ) n_g = 4 - 4 = 0 The relationship between K_p and K_c is given by: K_p = K_c( RT )^ n_g Substituting n_g = 0 : K_p = K_c( RT )^0 = K_c Therefore, K_p = 2.5 . Including solid species in the calculation would incorre