The entropy change for a reaction is -21.0 J/K.  If delta H is -10.0 kJ/mol, calculate Keq at 100o C using the Gibbs Free Energy equation and its relationship to Keq.

For a reaction   ΔH= -4.7 kJ  and  ΔS= -69.5 J/K at 25 oC.  Determine the ΔG for this reaction

Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH3(g) → 3 Ni(s) + N2(g) + 3 H20(g) If AG° = -18.1 kJ/mol, determine the value of AG assuming that a mixture contains 57.6 g of NiO, 182.3 g of Ni, 0.24 atm of NH3, 8.54 atm of N2 and 10.07 atm of H2O. kJ 1 2 3 4 6. C 7 8 9. +/- х 100 +

Which of the following statements define the third law of thermodynamics? O Process that requires continual input of energy from an external source Process that takes place without a continuous input of energy from an external source O All spontaneous processes involve an increase in the entropy of the universe O Entropy of a perfect crystal at absolute zero, or 0 K, is zero

Predict the normal boiling point of hydrogen peroxide (H2O2) from the following data:    ΔHºf, kJ/mol Sº, J/(mol • K) H2O2(ℓ)  –187.8  110 H2O2(g)  –136.3  233 Tb =  Based on the estimated boiling point, is H2O2 a liquid or a gas at room temperature (25°C)? Why?Choose one:A liquid, because its estimated boiling point is less than 25°C.A gas, because its estimated boiling point is less than 25°C.A liquid, because its estimated boiling point is greater than 25°C.A gas, because its estimated boiling point is greater than 25°C.

Define enthalpy, entropy and free energy. Include their chemical symbols in your explanation.

When 0.783 g of benzoic acid, C7H6O2 (122.12 g/mol) is burned in a bomb calorimeter, the temperature rises from 21.84 °C to 23.93 °C. If ΔE for the reaction is -3226 kJ/mol, what is the calorimeter constant of the calorimeter in kJ/°C? Please give your answer to two decimal places.

Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH (g)→3 Ni(s) + N,(g) + 3 H,O(g) | kJ If AG° = -18.1 kJ/mol, determine the value of AG assuming that a mixture contains 57.6 g of NiO, 182.3g of Ni, 0.24 atm of NH, 8.54 atm of N, and 10.07 atm of H,O. %3D 1 3 3 4 6. C 8. 9. +/- 0. x 100 2. 5

Using the tables, what is the standard Gibbs free energy change for the following reaction? CH4 (g) + 2 02 ( > CO2 (g) + 2 H2O (g) Report your answer in units of kJ, but do not type the units. Do not round your g) - answer.

Gibbs Free Energy is defined as: AGº ΔΗ-Τ. ΔS. Using the following data calculate Gibbs Free Energy for 1 mole of nitrogen gas. N2(g) AH O kJ/mol S° = 191.6 J/K'mol