Enthapy, ΔH = ΔE + PΔV is equal to q for reactions at constant pressure that   a. involve only solids   b. have gases as products, but not reagents   c. have gases as reagents, but not products   d. occur in aqueous solution

Calculate Delta G°rxn for the reaction: N2O(g) + NO2(g) -> 3NO(g) Given: 2NO(g) + O2(g) -> 2NO2(g)    Delta G°rxn = -71.2 kJ N2(g) + O2(g) -> 2NO(g)    Delta G°rxn = +175.2 kJ 2N2O(g) -> 2N2(g) + O2(g)    Delta G°rxn = -207.4 kJ

Consider the reaction A  -> 2 B. Suppose 2.50 mol of A is initially introduced into a 1.00 L flask. Equilibrium is established at 25 °C with a concentration of B of 0.11 mol L-1. What is the standard change in Gibbs free energy for this reaction?

What is the definition of standard condition when working with free energy? A. ions or molecules in solution at one molar concentration. B. both gases at one atmospheric and ions or molecules in solution at one molar concentration. C. gases at one atmosphere, ions or molecules in solution at one molar concentration and 0 K temperature. D. There’s no such thing as standard condition.

Mixture ΔT NaCl + H2O -0.2  NaNO3 + H2O -0.9 NaCH3COO + H2O 0.9   Which reactions are endothermic? Which are exothermic? What is the sign of enthalpy ΔH in each case? What is the sign of change in Gibbs free energy ΔG for each process in the forward direction? Could you predict the sign for entropy ΔS for these reactions? How could you tell the sign?

calculate ΔG rxn at 325 K for the hypothetical reaction below A2B8 (g) + 3O2 (g) ----> 2AO (g) ΔH°f (kJ/mol) -198 0 23 S° (J/mol•K) 281 205 180

A 0.318 M NaNO3 solution has a density of 1.02 g/mL. a. Does (pure) water or the solution have a higher standard entropy? Why? b. How much osmotic pressure does the solution exert at 25o C? c. Given that the pure water has a vapor pressure of 23.8 mm Hg, determine the vapor pressure of the solution.

For a certain chemical reaction, the standard Gibbs free energy of reaction at 25.0 °C is 116. kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K - ] х10

​ Determine ΔG°rxn for the following reaction:   N2O (g)  +  NO2 (g)  à  3 NO (g)​​ΔG° = ? Use the following reaction with known ΔG° values. ​Rxn 1:​​2 NO (g)  +  O2 (g)  à   2 NO2 (g)​​ΔG1° =  - 71.2 kJ​ ​Rxn 2:​​N2 (g)  +   O2 (g)  à   2 NO (g)​​ΔG2° =  + 175.2kJ Rxn 3:​​2 N2O (g)   à   2 N2 (g)  +   O2 (g)  ​​ΔG3° =  - 207.4kJ

Calculate the standard enthalpy, entropy, and Gibbs free energy at 298 K for the reaction shown, using the thermodynamic data in this table. 2 SO, (g) + 0,(g) → 2 SO, (g) kJ mol AHixn J K-mol ASixn kJ mol AGixn II