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?

1. Please consider 0.15 gm of Constantan (a Cu/Ni alloy widely used in thermocouples, c = 390 J/•K-kg) that cooled through exposure to the laboratory atmosphere (T 22 •C) from 620 C to 20 C. a. Please determine the change in entropy of the Constantan (in J/ K- kg). b. Please determine the change in entropy of the laboratory atmosphere (in J/ K-kg). c. Please determine the change in entropy of the universe (in J/ K-kg). %3D

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…

A chem.. ngineer 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 52.0 °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 J AS = 557. K N, (g) + 0, (g) → 2NO (g) AG = N, (g) + 0,(8) kJ Which is spontaneous? this reaction the reverse reaction neither ΔΗ - - 1353. kJ J AS = K 2CH,OH (g) + 30,(g)…

For the decomposition of mercury(II) oxide, HgO, to mercury and oxygen: 2H9O(s) → 2Hg() + O2(g) What is the standard change in entropy for this reaction? s° / J-mol-1.K-1 HgO(s) Hg() O2(9) 70.29 76.02 205.14 а. -1 210.87 J-K b. 58.83 J.K -1 c. 216.60 J-K -1 d. 351.45 J-K -1

Question 1

ouming Calculate the standard molar entropy of vaporization of water at 43.0 °C, given that its standard molar entropy of vaporization at 100.0 °C is 109.0 J-K mol and the molar heat capacities at constant pressure for liquid water and water vapor are 75.3 J-K1.mol-1 and 33.6 J-K.mol, respectively, in this temperature range. J.K-1. mol-1 ASvap TOOLS x10 Question Source: Atkins 7e - Chemical Principles | Publisher: W.H. Fm We The

llus_engine.html?ClassID=1653724337# Calculate the change in entropy for the reaction. H2(g) + l2(g) = 2HI(g) Substance S° (J/mol·K) H,(g) 1,(8) HI(g) 130.58 116.73 206.30 AS° = [ ? ] J/mol - K Enter either a + or - sign AND the magnitude in your answer. Enter

Calculate the change in the molar entropy of solid sodium chloride at constant pressure (1.00 bar) during heating from 0°C to 400°C. The constant-pressure molar heat capacity of NaCl(s) – which is not constant - takes the following form. 45.94 J 16.32 x 10-3 J T. Cp,m3 K mol K2 mol