A reversible reaction between hydrogen and iodine occurs as follows: H2(g)+I2(g)2HI(g)Kc=49.0at700K Where Kc is the equilibrium constant. (a) If a 10L reaction vessel is fed with 1 mole of H2 and 1 mole I2 at 700K, what are the equilibrium concentrations of all components? (b) If krr=1.20103M1s1 at 700K, what is the value of kf at the same temperature? Where kr is the forward reaction rate constant and krr is the reverse rate constant. (c) If the forward reaction is endothermic, explain with justification how an increase in temperature affects the values of Kc,kf and kr ? A reversible reaction between hydrogen and iodine occurs as follows: H2(g)+I2(g)2HI(g)Kc=49.0at700K Where Kc is the equilibrium constant. (a) If a 10L reaction vessel is fed with 1 mole of H2 and 1 mole I2 at 700K, what are the equilibrium concentrations of all components? (b) If krr=1.20103M1s1 at 700K, what is the value of kf at the same temperature? Where kr is the forward reaction rate constant and krr is the reverse rate constant. (c) If the forward reaction is endothermic, explain with justification how an increase in temperature affects the values of Kc,kf and kr