Calculate the change in Gibbs free energy for the reaction between hydrogen gas and iodine gas that forms hydrogen iodide gas. The balanced equation is as follows:H2(g) + I2(g) → 2HI(g)Assume a temperature of 298 K and use the following standard molar free energy of formation values:∆Gf° (HI) = -17.4 kJ/mol∆Gf° (H2) = 0 kJ/mol∆Gf° (I2) = 0 kJ/mol

Question

Calculate the change in Gibbs free energy for the reaction between hydrogen gas and iodine gas that forms hydrogen iodide gas. The balanced equation is as follows:H2(g) + I2(g) → 2HI(g)Assume a temperature of 298 K and use the following standard molar free energy of formation values:∆Gf° (HI) = -17.4 kJ/mol∆Gf° (H

Answer 1

To calculate the change in Gibbs free energy for the reaction, we can use the following equation:G =  Gf products  -  Gf reactants For the given reaction:H2 g  + I2 g   2HI g The products are 2 moles of HI and the reactants are 1 mole of H2 and 1 mole of I2. Using the provided standard molar free energy of formation values, we can plug them into the equation:G = [2 *  -17.4 kJ/mol ] - [ 0 kJ/mol  +  0 kJ/mol ]G =  -34.8 kJ/mol  -  0 kJ/mol G = -34.8 kJ/molThe change in Gibbs free energy for the reaction between hydrogen gas and iodine gas that forms hydrogen iodide gas is -34.8 kJ/mol.