1. You are interested in formic acid as a chemical storage medium for hydrogen and are studying the vapor phase decomposition of formic acid, HCOOH, into molecular hydrogen H2 and carbon dioxide CO2. You may assume ideal behavior of the vapor: HCOOH(g)>H2(g)+FO2(g) The standard Gibbs energy of formation of formic acid (g) is g=351kJ/mol and the standard enthalpy of formation is h=379kJ/mol. (a) Calculate the standard Gibbs energy of reaction for the decomposition in kJ/mol. (b) Calculate the standard reaction equilibrium constant. (c) Calculate the enthalpy of reaction in kJ/mol (d) Calculate the equilibrium constant at a temperature of 50C assuming that the enthalpy of reaction is not a function of temperature in this interval. (e) Calculate the extent of reaction in mol under standard conditions using a starting amount of 1 mol formic acid. (f) Calculate the extent of reaction in mol at a temperature of 50C and 1 bar using a starting amount of 1mol formic acid