For a certain chemical reaction, the standard Gibbs free energy of reaction at 10.0 °C is 137. kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. 00 K = ? do

For a certain chemical reaction, the equilibrium constant K = 4.5 × 10 - 10 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. %3D Round your answer to 2 significant digits. AG° = | kJ |x10

For a certain chemical reaction, the equilibrium constant K = 1.9 × 10¯¯ at 5.00 °C. Calculate the standard Gibbs free energy of reaction. -4 Round your answer to 2 significant digits. AG° = | KJ x10 ? X Ś

4. The entropy change for a reaction is zero.  If the delta H is -10.0 kJ/mol, calculate Keq using the Gibbs free energy equation and its relationship to Keq at 100 degrees Celsius. 5. Predict whether the entropy change will be positive or negative for the following reaction.  Justify your answer.   H2C=CH2  +  2 O3    =    6 CH2O   6. In THF, which is miscible with water,the kinetics are first order in both reactants for the following reaction:   C3H7-Br  +  H2O    =    C3H7-OH  +  HBr If the concentration of C3H7Br is set at 0.200 M, use the following time-concentration data to calculate the first order rate constant for water: time in minutes   M H2O                 0             2.00x10exp-3                3              1.87x10exp-3