ed under standard conditions, when the reaction is st ate the non-standard Free Energy change (AG) at 298 s of the three gases. Answer in kJ. 1) at 298 K partial pressure (atm) N2 1.0 H2 0.06 NH3 1.5

10. How much energy is given off when 1.00 g Fe is reacted with excess oxygen? 4Fe(s)302(g)-»2Fe2O3(g) AH -1652 kJ а. 14.8 kJ b. 3.70 kJ c. 7.39 kJ d. 1179 kJ е. 589 kJ

193.) The standard free energy change = blank

A student determines the value of the equilibrium constant to be 7.49×10-37 for the following reaction. H,S(g) + 2H2O(1)3H2(g) + SO2(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.03 moles of H,S(g) at standard conditions at 298K. AG. rxn kJ

The difference in standard free energy between reactant R and product P is + 7.5 kJ/mol. What’s the ratio of P to R at equilibrium? P to R ratio =

Consider a chemical reaction where AS is 40.0 J/K, and AH is 25.0 kJ. What is the change in free energy (AG) for this reaction at 298K? O-22.4 kJ 3.9 kJ O 65.9 kJ O-37.9 kJ O 13.1 kJ

1)State the First Law of Thermodynamics.                                               2)Fluorine (F2) and iodine (I2) are both Group 17 elements. Explain with reference to intermolecular forces, why fluorine is a gas and iodine is a solid at room temperature.                                                                                                                                                                                       4)When 30 g of ammonium nitrate, (NH4NO3) was stirred into 10 cm3 of water, the temperature fell from 21 oC to 15 oC.   5)Calculate the total amount of energy (E) released in this experiment. Ignore the heat capacity of ammonium nitrate. Take the specific heat capacity of the water as 4.18 J g-1 ºC-1. Density of water is 1.00 gcm-3.                                             6)This amount of energy [answer to part (i)] was produced by 30 g of ammonium nitrate.  Calculate the energy change per mole of ammonium nitrate.  Include the correct sign for…

At 25°C, the free energy of formation of gaseous water is -229 KJ/mole. Calculate ΔG (in KJ) for the following reaction if the hydrogen is supplied at 4.00 atm and the oxygen is supplied at 3.00 atm, while the water produced is at 1.00 atm pressure?

Given the following two measurements of the equilibrium constant for a reaction, calculate ΔH° for the reaction. (kJ/mol) T, °C                   K 30.0                5.2 x 103 50.0                15.4 x 104

The enthalpy change (A,H) of the following reaction, generating 1 mol O₂(g), at 25°C and 1.00 atm is +290.8 kJ. 2ZnO(s) + 25(s)--> 2ZnS(s)+O₂(g) What is the energy change (A,U) of this reaction? 293.3 kJ 288.3 kJ 2.48 KJ -2.48 kJ McQuarrie and Simon Example 5-7 and Eq. 5.38