For the following reaction (the detonation of nitroglycerin), is it spontaneous under standard conditions and how can you tell? 4 C4H5N3O9(l) (arrow >) 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)    ΔH = -5678 kJ

For a particular reaction, ΔH = -32 kJ and ΔS = -98 J/K.Assume that ΔH and ΔS do not vary with temperature.(a) At what temperature will the reaction have ΔG = 0?(b) If T is increased from that in part (a), will the reactionbe spontaneous or nonspontaneous?

For the reaction Fe,03(s) + 2Al(s) Al,O3(8) + 2Fe(s) AH° - -851.5 kJ and AS° = -37.0 J/K %3D The maximum amount of work that could be done when 2.36 moles of Fe,03(s) react at 338 K, 1 atm is kJ. Assume that AH° and AS° are independent of temperature.

The decomposition of copper (1) oxide to its elements does not occur spontaneously at 375°C (AG = 140.0 kJ): Cu₂0 (s) 2 Cu (s) + 1/2O₂(g). It can be made to occur spontaneously by being coupled to the oxidation of solid carbon to form carbon monoxide gas at this same temperature (AG = -143.8 kJ): C(s) + 1/2O₂(g) → CO (g) What product(s) is/are produced as a result of coupling the two reactions? CO (g) 2 Cu (s) and 1/2 O₂ (g) 2 Cu (s) and CO (g) 2 Cu (s), 1/2 O2 (g), and CO (g) 1/2 0₂ (g)

A mole of sodium met is added to water How much work is done on the atmosphere by the subsequent reaction if the temperature is 25 C°

A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 74.0 °C and constant total pressure. Then, he 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 his 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 = 181. kJ AS = -499. K ? 2NO(g) N, (g) + 0, (g) AG = kJ Which is spontaneous? this reaction the reverse reaction neither

Under what temperature conditions (low T, high T, all T, nonspontaneous at all T) would this reaction occur spontaneously? Explain your reasoning. 2NH4NO3(s) → 2N2(g) + 4H2O(l) + O2 (g)  , ∆Horxn = -236.0 kJ

"M" represents a metallic element.  "X" represents a nonmetallic element.  Calculate ΔH for the process M3X4(s) ⟶ 3M(s) + 2X2(g) from the following information: M(s) + ½X2(g) ⟶ MX(s)  ΔH°= -286.2 kJ 3MX(s) + ½X2(g) ⟶ M3X4(s)  ΔH°= -84.3 kJ

In each of the following, use the tables of ΔHo and So to calculate ΔGo at 298 K for the reaction equation as given. 1. N2(g) + 3H2(g) → 2NH3(g) 2. Cu(s) + 1⁄2O2(g) → CuO(s)

For the reaction C(s,graphite) + 02(g) CO2(g) AG° = -394.3 kJ and AS° = 2.9 J/K at 290 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 290 K. The standard enthalpy change for the reaction of 2.38 moles of C(s,graphite) at this temperature would be kJ.