SnO2(g) + 2C(s) = Sn(s) + 2CO2(g) AH =+ 360.0 KJ Pressure is decreased N2(g) + 3 H2(g) 22 NH3(g) 4H = -92 kJ mol-! the solution is cooled some AgNO; is added to the solution AgCl(s) = Ag*(aq) + Cl-(aq) N2(g) + 3 H2(g) =2 NH3(g) pressure is increased

Consider the following reaction: 3C(s) + 3H2(g) - C3H68); AG° - 60.0 kJ and AS" --256.7 J/K at 298 K What is the equilibrium constant and AH° at 298 K for this reaction? Express AH° in kJ and use 3 significant figures for both answers. AH° - kJ and Keq' x 10

A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 59.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 852. kJ J AS = 2645. K Al, 0, (s) + 2Fe(s) → 2A1(s) + Fe,0, (s) AG = | kJ Which is spontaneous? this reaction the reverse reaction neither

1. A student determines the molar mass of acetone, CH,COH., by the method used in this experiment. She found that the equilibrium temperature of a mixture of ice and water was 0.5°C on her thermometer. When she added 10.5 g if her sample to the mixture, the temperature, fell to -2.6°C. She then poured off the solution through a screen into a beaker. The mass of the solution was 86.4g. d. How much water was in the decanted solution?