Sulfur has two solid forms - a (or rhombic) and b (or monoclinic). The standard enthalpies...
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.
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?
Enthalpy of Formation Part 1: Part 2: Part 3: A scientist measures the standard enthalpy change for the following reaction to be 591.0 kJ : 2H2O(1)—>2H2(g) + O2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(l) is kJ/mol. A scientist measures the standard enthalpy change for the following reaction to be -2903.4 kJ: 2C2H6(g) + 7 O2(g)—>4CO2(g) + 6 H2O(g) Based on this value and the standard...
A scientist measures the standard enthalpy change for the following reaction to be -1064.8 kJ: 2H2S(g)3 O2(g> >2H2O(g) 2 S02(g) kJ/mol Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of S02(g) is A scientist measures the standard enthalpy change for the following reaction to be -138.6 kJ H2(g)C2H4(g) C2H6(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of...
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=...
Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: 2HCI(g) + Br2(g)>2HBr(g) + Cl2(g) kJ Submit Answer Retry Entire Group 9 more group attempts remaining Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction 2H2(g) +o2(g) 2H2O(g) kJ Submit Answer Retry Entire Group 9 more group attempts remaining
Anhydrous ammonia is an ultra-clean and energy-dense alternative fuel that produces no greenhouse gases on combustion. In an experiment, gaseous ammonia is burned with oxygen in a container of fixed volume per the following equation: 4NH3(g) + 302(g) -> 2N2(g) 6H20(0) The initial and final states are at 298 K. After combustion with 12.80 g of O2, some NH3 remains unreacted. Calculate the enthalpy change during the process, given the following data. | ?,Ho (KJ mol-1) compound NH3 (g) H20...
Part A Several reactions and their standard reaction enthalpies at 298.15 K are given here: Al_C3(s) + 12H2O(l) + 4Al(OH),(s) + 3CH4(g) 2Al(s) + O2(g) + Al2O3(s) 1 A1,03(s) + H2O(l) + Al(OH)3(s) AH (kJ. mol-?) –1683.0 -1675.7 -9.6 The standard enthalpies of combustion of graphite and CH4(8) are -393.51 and --890.35 kJ. molº respectively. Calculate the standard enthalpy of formation of Al4C3(s) at 25°C.
Question 7 Use the standard reaction enthalpies given below to determine AHºrxn for the following reaction: 4 503 (g) ==> 4 S (s) + 6 O2 (g) AHºrxn = ? GIVEN: SO2 (g) ==> 5 (s) + O2 (g) AHºrxn = 436 kJ/mol 2 SO2(g) + O2 (g) ==> 2 503 (g) AHºrxn = -1,019 kJ/mol Report your answer to 4 sig figs. Question 8 If 531 mL of gas is obtained at 65.0°C by collecting CO gas over water...
9. Given the following bond enthalpies, calculate the AHxn for the following reaction. 1. C2H4 + 302 > 2cO2 + 2H20 BOND C-H С-О о-н 0-0 с-с Bond Enthalpy (kJ/mol) 413 799 463 495 614 10. Match the following molecules with their type of bonding: non-polar covalent, polar covalent, or ionic. a. MgCl2 b. HClc. Clz