As a fuel, H2(g) produces only non-polluting H2O(g) when it burns. Moreover, it combines with O2(g) in a fuel cell to provide electrical energy. a) Calculate ΔHosys, ΔSosys, and ΔGosys per mole of H2(g) at 298K. b) Is the spontaneity of this reaction dependent on T? c) At what temperature does the reaction become spontaneous?

A helium-filled balloon at 1.00 atm pressure has a volume of 1.410 L. It is placed in a freezer and its volume decreases, stopping at 0.960 L.(Assume that the static internal and external pressures are equal, that the balloon contains only helium, and helium behaves as an ideal gas.)Calculate ΔE for the gas in the balloon.

For the reaction below, calculate the value of the temperature at which the reaction becomes spontaneous, and is it spontaneous above or below that temperature?4 Ca3PO4 (s)  +   3 O2 (g)    →    12 CaO (s)   +   P4O10 (s)  Delta H=+5946.8  Delta G=+5656  Delta S= – 9.80 x 10^2  Select one: a. 6.07 x 10^3 K, and spontaneous above this temperature b. 6.07 x 10^3 K, and spontaneous below this temperature c. 16.3 K, and spontaneous above this temperature d. 16.3 K, and spontaneous below this temperature e. 16.3 ℃, and spontaneous above this temperature f. 16.3 ℃, and spontaneous below this temperature g. this reaction is always spontaneous. h. this reaction is never spontaneous! i. none of these.

Use thermodynamic values in the table provided to calculate the ΔG for the following process in two ways.                    4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) at 25˚C   a) Use Free Energy values to calculate ΔG. b) Use Enthalpy and Entropy values with Gibbs Equation to calculate ΔG. c) What do your final ΔG values tell us about this reaction?

Please help with # 39. I do not know how to solve

Arrange the following from lowest to highest entropy: Licl(s) NaBr(s) KI(s) LiF(s)

Consider the formation reaction of water, the hydrogen balloon reaction: 2 H,(g) + 0,(g) → 2 H,0(g) Which ONE of the following statements is FALSE for this reaction? ΑΔΗ<0 В AS < 0 The reaction is spontaneous at all C temperatures. AG = 0 at some very high D temperatures.

For the following example, identify the following:   F2(l) → F2(g)   A. at low temperature, the reaction is spontaneous and ΔG < 0 and at high temperature, the reaction is spontaneous and ΔG < 0 B. at low temperature, the reaction is nonspontaneous and ΔG > 0 and at high temperature, the reaction is spontaneous and ΔG < 0 C. at low temperature, the reaction is spontaneous and ΔG < 0 and at high temperature, the reaction is nonspontaneous and ΔG > 0 at low temperature, the reaction is nonspontaneous and ΔG > 0 and at D. high temperature, the reaction is nonspontaneous and ΔG > 0 It is not possible to determine without more information.

17.28 From each equation and standard enthalpy, predict whether the reaction will be spontaneous at all temperatures, spontaneous at low temperatures but nonspontaneous at high temperatures, nonspontaneous at low temperatures but spontaneous at high temperatures, or not spontaneous at any temperature. Explain the reasons. (a) 2HgO(s) 2Hg(l) + O2(g) = 90.8 kJ → (b) 4Fe(s) + 302(g) → 2Fe2O3(s) AH = -1648.4 kJ (c) N2(g) + 3Cl2(g) → 2NC13(g) днө — 460 kJ 作答 (d) 2NH4NO3(s) → 2N2(g) + 4H2O(g) + O2(g) AH® = -225.5 kJ

At 1200 oC, the reduction of iron (III) oxide (Fe2O3) to elemental iron is not spontaneous: 2Fe2O3(s) → 4Fe(s) + 3O2(g) rG° = +840 kJ At the same temperature solid carbon spontaneously reacts with oxygen, to form CO2 gas. It is found that by mixing carbon with Fe2O3 at this temperature the reduction can be made to proceed, providing at least 3 moles of carbon are present for every 2 moles of Fe2O3. (a)write a balanced equation for the total reaction (b) Use the reaction stoichiometry to determine an upper limit for rG, i.e. the least negative value possible, for the reaction of carbon with oxygen at this temperature. (+840 is the only delta G value given in the question)