Calculate ΔS for the mixing of 20.0 g of He at 120°C and 1.50 bar with 10.0 g of O2 at 120°C and 1.50 bar. Find dS for this process in J/K
Calculate ΔS for the mixing of 20.0 g of He at 120°C and 1.50 bar with...
Calculate ΔS∘rxn for the reaction 2NO(g)+O2(g)→2NO2(g) Substance S∘ (J/mol⋅K) NO2 240.0 O2 205.2 NO 210.8
For the following reaction: 2 CO(g) + O2(g) → 2 CO2(g), given ΔH = -566 kJ and ΔG = -514 kJ, find ΔS (J/K) at 25 oC. Multiple Choices: ΔS = -174 J/K ΔS = -0.174 J/K ΔS = -2.08J/K ΔS = 174 J/K ΔS = -2080 J/K
One mole of O2(g), with CV,m=2.5R, is expanded adiabatically from 301 K and 4.00 bar to 1.60 bar against a constant external pressure equal to the final pressure. Calculate q, w, ΔU, ΔH, ΔS and ΔSsurr. Enter your answers in the specified units with three or more significant figures . Do not include units as part of your answer. q = ____________ J w = ____________ J ΔU = ____________ J ΔH = ____________ J ΔS = ____________ J mol-1 K-1...
Calculate ΔS∘rxn for the following balanced chemical equation: 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance and state S∘[J/(K⋅mol)] H2O(g) 188.8 O2(g) 205 H2S(g) 205.7 SO2(g) 248.1
22 g of Co, gas is in a container under 1.50 bar. After isothermal reversible expansion, volume of the gas changes from 2 dm to 5 dm'. Calculate the change in the system's entropy? (C: 12 g/mol; O: 16 g/mol) (R-8.314 1/mol.) A-) 6.69 J/K B-) 335.2 J/K C-) 3.81 J/K D-) 0.458 J/K E-) 167.6 J/K
For the values give for ΔH and ΔS, calculate ΔG foreach for each of the following reactions at 298 K. If the reactionis not spontaneous under standard conditions at 298 K, at whattemperature (if any) would the reaction become spontaneous? a) 2PbS(s)+3O2(g) ---> 2PbO(s)+2SO2(g) ΔH= -844kj ; ΔS = -165 J/K b)2POCl3(g)--->2PCl3(g)+O2(g) ΔH= 572kJ ; ΔS= 179 J/K
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
Calculate ΔS∘rxn for the balanced chemical equation H2S(g)+2O2(g)→H2O(g)+SO3(g) Express the entropy change to four significant figures and include the appropriate units. Standard enthalpies for selected substances at 25∘C Substance S∘(J/(mol⋅K)) O2(g) 205.2 SO2(g) 248.2 SO3(g) 256.8 H2O(g) 188.8 H2S(g) 205.8
Consider the following reaction: 2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K Calculate the free energy change for the reaction at 32 ∘C.
Use the data in Appendix B in the textbook to calculate ΔH∘ and ΔS∘ for each of the following reactions. From the values of ΔH∘ and ΔS∘, calculate ΔG∘ at 25 ∘C and predict whether each reaction is spontaneous under standard-state conditions. Part A 2SO2(g)+O2(g)→2SO3(g) Express your answer using four significant figures. ΔH∘ = kJ Part B Express your answer using four significant figures. ΔS∘ = J/K Part C Express your answer using four significant figures. ΔG∘ = kJ Part...