The integrated form of Kirchhoffs Law. A,H(T2) = A, H(T;) + A, Cp(T2 - T) where A,H(T;) and A,H(T2) are the reaction enthalpies at temperatures T;and Tz respectively and A,Cp is the heat capacity of the reaction works based on the assumption that: A. For extremely large temperature changes, the heat capacity of the reaction can be assumed independent of temperature. B. For extremely large temperature changes, the heat capacity of the reaction increases linearly as a function of temperature C. For extremely small temperature changes, the heat capacity of the reaction can be assumed independent of temperature D. For extremely small temperature changes, the heat capacity of the reaction increases linearly as a function of temperature O E. Both (B) and (C)

For the reaction P4010(s) + 6 H20(1) 4 H3PO4(aq) AG° = -448.9 kJ and AS° = -16.3 J/K at 261 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 261 K. The standard enthalpy change for the reaction of 2.15 moles of P4010(s) at this temperature would be kJ. Submit Answer Try Another Version 1 item attempt remaining rch a

Calculating dG from dH and dS 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. alo AH = -172. kJ J AS = -420. K CH, OH (g) + CO(3) - HCH,CO, (1) AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither AH =…

Gaseous SO2Cl2 reacts with liquid water to form hydrogen chloride gas and liquid sulfuric acid. Using data tabulated in Appendix G of your text, calculate the enthalpy change, in units of kJ/mol, for the formation of 2 mol of liquid sulfuric acid.

3. Heats of reaction can also be calculated using heats of formation and the relationship - AHrxn = ΣnAHƒ.prod — ΣmAHƒ.reac Substance HCl(aq) MgCl2(aq) MgO(s) H₂O(/) H.(kJ/mol) -167.2 -796.8 -601.2 -285.8 0 a. Standard State Elements Calculate the theoretical AH° values for the following reaction Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) Mg(s) + O2(g) → MgO(s)

P2C.6 For the reaction Cr(C,H,),(s) → Cr(s) +2OC,H,(g), A̟U°(583 K) = +8.0 kJ mol'. Find the corresponding reaction enthalpy and estimate the standard enthalpy of formation of Cr(C,H),(s) at 583 K. %3D

V:OY IA %YA N& 令 l PNG.9 → حداد H.W) calculate AçH° (500 K) for methane by using the data given on the temperature dependence of heat capacities. CH4(g)+2O2(g)→CO2(g)+2H2O(g) AÇH° (298 K) -891 kJ Cp,m(CO2) = 44.22 + 8.79 × 10-37 - 8.62 × 105 T2 Cp.m(H2O) = 75.29 + 0 + 0 Cp,m(O2) = 29.96 + 4.18 × 10-37 1.67 × 105 T2 Cp,m(CH4) = 35.31

A quantitity of 100mL of 0.500 MHCl was mixed with 50 mL of 0.500M NaOH in a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and NaOH solutions was the same, 20ºC, and the final temperature of the mixed solution was 22.3ºC. Calculate the heat change for neutralization reaction on a molar baisis.

3) Calculate the reaction heat of formation of PbO from Pb and O2 at rxn temperatures of 500K and 800K seperately (using below reactions). Pb(s) + 1/2 O2(g) Pb(1) + 1/2 O2(g)- AH°298.PbO =-219400 J/mole Cp (PbO.s)-52.3 +8.66 x 10T- 8.2x10 T J/molK (298-1159 K) CP (Pb.s)-24.3 +8.7 x 10 T Cp (Pb.)= 32.5-3.1 x 10 T Cp(02g)-29.9 +4.18 x 10 T-1.7x10 T2 Pb(s)→ PbO(s) PbO(s) J/molK (298-600 K) J/molK (600-1300 K) J/molK (298-2500 K) Pb(1). AHmelting 4800 J/mole, Tmelting 600K

(d) The enthalpy change for the reaction (A,Hº) of ethyne (C,H,) is -2511.6 kJ. i. Write a balance equation for the combustion of ethyne. ii. Determine the enthalpy of formation A¡Hº of ethyne given the following: A¢H° CO2 = -393-5 kJ mol" A¡Hº H2O_ = -241.8 kJ mol" A¡H° O2 = 0.00 kJ mol-1 %3D