4. Consider the reaction 3 C (graphite)2 H2O (g) CH4 (g) 2 CO (g) The following...
For the reaction Co (g) + 3 H2 (g)CH4(g) + H2O (g) calculate the enthalpy change in kJ at standard temperature and pressure for the consumption of 1.2 moles of carbon monoxide (g). The table below gives thermodynamic parameters. compound at 25 C ΔΗ f kj mol 'S JK ' mol kj mol carbon monoxide (g) -110.53 hydrogen (g) methane (g) water (I) water (g) 0 -1 197.67 130.68 186.26 69.95 188.83 137.17 74.81 285.83 241.82 -50.72 237.13 228.57 rxn...
Predict the signs, comment and then calculate the enthalpy and entropy changes for the reaction of combustion ofmethane at 500 K. Will the reaction be spontaneous at 500 K? CH4(g) + 2 O2(g) → CO2(g) + 2H2O(g) We give: The enthalpies of formation of the products at 298.15 K in kJ/mol are: ∆Hf(CO2) = - 393.51; ∆Hf(H2O) = - 241.82; ∆Hf(CH4) = -74.81. The heat capacities at constant pressure in J.mol-1.K-1: Cp(CO2) = 37.11; Cp(H2O) = 33.58; Cp(CH4) = 35.31;...
Consider the reaction at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ Calculate the quantities. Delta Ssys=_______ J/K Delata Ssurr =_______ J/K
Consider the following reaction at 298 K.C(graphite) + 2H2(g)→ CH4(g) ΔH°=-74.6 kJ
Consider the following reaction at 298 K. C(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/KC(graphite)+2H2(g)⟶CH4(g)ΔH∘=−74.6 kJ and ΔS∘=−80.8 J/K Calculate the following quantities. ΔSsys=ΔSsys J/K ΔSsurr= J/K ΔSuniv= J/K
Using the following data determine the temperature (in K) at which the reaction H2O(g)+ C(s,graphite) ↔ H2(g) + CO(g) this becomes spontaneous. ΔfH° (H2O(g)) = -251.2 kJ mol-1 ΔfH° (C(s,graphite)) = 0.0 kJ mol-1 ΔfH° (H2(g)) = 0.0 kJ mol-1 ΔfH° (CO(g)) = -110.1 kJ mol-1 S° (H2O(g)) = 192.6 J K-1 mol-1 S° (C(s,graphite)) = 6.4 J K-1 mol-1 S° (H2(g)) = 136.9 J K-1 mol-1 S° (CO(g)) = 192.4 J K-1 mol-1
4. Using the information in the data table provided, a.Predict what physical state PCl3 is in at 298 K. b. Estimate the boiling point of PCl3. You may assume that deltaH and deltaS do not vary with temperature (usually a reasonable assumption). AH+ (kJ/mol) 30.71 Sº (1/K*mol) 245.3 AG+ (kJ/mol) 3.14 52.30 219.4 68.11 -235.1 282.7 - 168.5 0 222.96 0 0 202.7 0 130.58 0 Brz (g) CH. (g) C2H5OH (g) Cl2 (g) F2 (g) Hz (g) HBr (8)...
A reaction to produce “substitute natural gas” is described by: 4 CO (g) + 8 H2 (g) → 3 CH4 (g) + CO2 (g) + 2 H2O (l) Use the following information, as necessary, to estimate DH for the above reaction. 2 C (graphite) + O2 (g) → 2 CO (g)ΔfH= –221.0 kJ/mol 2 CO (g) + O2 (g) → 2 CO2(g)ΔrH= –566.0 kJ/mol 2 H2 (g) + O2 (g) → 2 H2O (l)ΔfH= –571.6 kJ/mol C (graphite) + 2...
Consider the reaction Al2O3(s) + 3C(graphite) + 3Cl2(g) → 2AICI3(s) + 3CO(g) Determine the following at 298 K: X kJ/mol J/mol-K kJ/mol дно- What is log K at 298K (log K-In K/2.3026)? log K (Hint log K-(In K)/2.3026) Assume that ΔΗο and ΔSo are temperature independent to determine the following at 600 K. kJ/mol log K (log K = In K/2.3026)
Consider the following reaction at 298 K. AH' - -74.6 kJ and AS C(graphite) + 2 H2(g) - CH (8) Calculate the following quantities. -80.8 J/K ASxys - + TOOLS AS univ- X10 Is this reaction spontaneous? Ово O yes