From the following data, calculate the Enthalpy when Rhombic Sulphur is covered to monoclinic Sulphur
S (rhombic) + O2 (gas) -----> SO2 (gas) delta H = -295.1 kJ/mol
S (monoclinic) + O2 -------> SO2 (gas) delta H = -296.4 kJ/mol
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S (rhombic) -------> S (monoclinic) delta H = [x] kJ/mon
S (rhombic) + O2 (g) -----> SO2 (g) ,delta H = -295.1 kJ/mol -------------------------------equation 1
S (monoclinic) + O2 (g)-------> SO2 (g) ,delta H = -296.4 kJ/mol -------------------------------equation 2
subtract equation 2 from equation 1:
From the following data, calculate the Enthalpy when Rhombic Sulphur is covered to monoclinic Sulphur S...
10. Elemental sulfur exists in two crystalline forms, rhombic and monoclinic. From the following data = S(monoclinic) 5° (J/K mol) 31.880 S (rhombic) AHP (kJ/mol) S (rhombic) S(monoclinic) 0.30 a. Calculate the enthalpy change 32.546 b. Calculate the entropy change C. Calculate the Gibbs free energy at 25°C.
9.Enter your answer in the provided box. S(rhombic) + O2(g) → SO2(g) ΔHo rxn= −296.06 kJ/mol S(monoclinic) + O2(g) → SO2(g) ΔHo rxn= −296.36 kJ/mol calculate the enthalpy change for the transformation S(rhombic) → S(monoclinic) (Monoclinic and rhombic are different allotropic forms of elemental sulfur.) _______kJ/mol 10. Enter your answer in the provided box Use the following data to calculate ΔHo/f for CS2(l): C(graphite) + O2(g) → CO2(g) ΔHo rxn= −393.5 kJ/mol S(rhombic) + O2(g) → SO2(g) ΔHo rxn=...
Consider the phase transition between two phases of sulfur S(s, rhombic) S (s, monoclinic) IF AG for this transition is +0.10 kJ/mol and the densities of the rhombic and monoclinic phases are, respectively, 2.07 g/cm and 1.92 g/cm', at what pressure does the phase transformation from rhombic to monoclinic become spontaneous?
to P4.22 Calculate the standard enthalpy of formation of FeS2(s) at 550.°C from the data tables and the following data at 298.15 K. Assume that the heat capacities are independent of temperature. Substance Fe(s) FeS2(s) Fe2O3(s) S(rhombic) SO2(g) AfHⓇ (kJ mol-l) -296.81 Cp.m/R 3.02 7.48 2.72 -824.2 You are also given that for the reaction 2FeS2(s) + 11/202(g) ► Fe2O3(s) + 4802(g), A,Hº = -1655 kJ mol-!
Calculate the standard enthalpy of formation of CS2() given that AH=-393.5 kJ/mol AHo = -296.4 kj/mol a. C(s) + O2(g) CO2lg) b. S(s) +O2(g). SO2(g) AH = -1073.6 kj/mol C. CS2(I)+302(g) Co2lg) + 2S02(B)
7- (15 pts) Calculate the standard enthalpy of formation of CS2 (1) given that a. C(s) + O2(g) + CO2(g) b. S(s) + O2(g) → SO2(e) C. CS2() + 302(g) → CO2(g) + ' 250 (6) AH° = -393.5 kJ/mol AH° = -296.4 kJ/mol AH° = -1073.6 kj/mol (the standard state of the element Sulfur is S(s))
TC04M01 Use the enthalpy changes given in the data below to calculate the enthalpy change for this reaction: Cus(s) + O2(g) → Cu(s) + SO2(9) Data: Reaction no. Reaction A.HⓇ/kJ morat 298K standard state = 1 bar. +314 2 2 CuO(s) – 2Cu(s) + O2(g) S(s) + O2(g) - S02(9) 2CuO(s) + 2S(s) - 2CuS(s) + O2(9) -297 +208 Select one: a. +225 kJ/mol b.-85 kJ/mol O C. -244 kJ/mol d. -191 kJ/mol e. -225 kJ/mol
Calculate the Enthalpy of a reaction C + 1/2 O2 -----> CO2 , delta H = -110.3 kJ/mol CO + 1/2 O2 -----> CO2 , delta H = -283.2 kJ/mol _______________________________________ C + O2 -----> CO2 , delta H = [x] kJ/mol
Using the standard heats of formation that follow, calculate the standard enthalpy change for the following reaction. S(s,rhombic) + 2CO(g)— SO2(g) + 2C(s,graphite) AH°rxn- KJ Species AH®(kJ/mol CO(g) -110.5 SO2(g) -296.8 Check & Submit Answer Show Approach
Calculate the standard enthalpy change for the following reaction 2Al_2O_3(s) + 3C(s) rightarrow 4Al + 3CO_2(g) given the following: delta H CO_2(g) = -393.5 kJ/mol delta H C(s) = 0 kJ/mol delta H Al = 10.79 kJ/mol delta H Al_2O_3(s) = -1675.7 kJ/mol