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Consider this reaction between solid iron and water vapor. 3 Fe(s) + 4 H20(g) - Fe304(s) + 4 H2(g); OH = —151.2 kJ/mol When chemical systems are subjected to stresses, the equilibrium position may shift toward the reactants or products, or it may be unaffected. How would each of the following changes affect this equilibrium? (a) increasing the temperature shifts the reaction toward the reactants shifts the reaction toward the products does not affect equilibrium (b) adding Fe shifts the reaction toward the reactants shifts the reaction toward the products does not affect equilibrium (c) increasing the volume of the container shifts the reaction toward the reactants shifts the reaction toward the products does not affect equilibrium (d) increasing [H2O] shifts the reaction toward the reactants shifts the reaction toward the products does not affect equilibrium (e) increasing the pressure (and decreasing the volume) on the system shifts the reaction toward the reactants shifts the reaction toward the products does not affect equilibrium