The heat capacity at 1 atm. pressure of solid magnesium in the temperature range from 0 oC to 560 oC, is given by the expression: Cp = 6.20 + 1.33 x 10-3 T + 6.78 x 104 T-2 Cal. deg.-1 g. atom.-1 What is the increase of entropy per g. atom, for an increase of temperature from 300 K to 800 K at 1 atm. pressure?

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 26.0 °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. N₂(g) + 3H₂(g) → 2NH₂(g) P₁(s) + 20HF (g) 4PF, (g) + 10H₂(g) ΔΗ = -92. kJ AS = AG = | KJ -294. ΔΗ Which is spontaneous? this reaction the reverse reaction neither AS = = - 1005. kJ…

7. Consider the following process, in which AH® is 44.0 kJ/mol at 25°C and 40.6 kJ/mol at 100 °C H2O() → H2O(g) (a) If the entropy S for H2O(1) and H2O(g) are 70.0 J.mol.K' and 188.9 J.mol'.K', respectively, calculate AS.gys and ASsurr, each with appropriate algebraic sign at 25°C and at 100 °C. (b) Calculate ASuniv at 25°C and at 100 °C, and predict whether the evaporation of water is spontaneous at each temperature if PH20 = 1 atm.

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 69.0 °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. HCH, CO₂(1)→ CH₂OH(g) + CO(g) Al₂O₂ (s) + 2Fe(s) -> 2A1(s) + Fe₂O₂ (s) AH = 172. kJ AS = 543. AG = Which is spontaneous? O this reaction O the reverse reaction Oneither ΔΗ = 852. kJ…