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- Compound Δ?∘f (kJ/mol)ΔGf∘ (kJ/mol) A +387.7+387.7 B +600.4+600.4 C +402.0+402.0 Use the data given here to calculate the values of Δ?∘rxnΔGrxn∘ at 25 ∘25 ∘C for the reaction described by the equation A+B↽−−⇀C A+B↽−−⇀CA+B↽−−⇀C Δ?∘rxn=ΔGrxn∘= kJkJ If Δ?∘rxnΔHrxn∘ and Δ?∘rxnΔSrxn∘ are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is enthalpy-driven to the left. enthalpy-driven to the right. entropy-driven to the right. entropy-driven to the left.What is the ∆G◦ (in kJ mol−1) for the followingreaction at 25 ◦C?NO2(g) ⇌ N2O4(g)NO2(g):∆H◦ = 33 kJ mol−1; S◦ = 240 J mol−1 K−1N2O4(g):∆H◦ = 11 kJ mol−1; S◦ = 304 J mol−1 K−1A. −41.1 B. −8.8 C. −2.5 D. 16.2E. 5.24 × 1046. Use Appendix G (Links to an external site.). to calculate ΔS°rxn for the following reaction. N2(g) + 3H2(g)<=> NH3(g) Group of answer choices A, -198.5 J/K B, 185.5 J/K C, 198.5 J/K D, 198.5 kJ/K mol E, -198.5 J/ mol 7. Use Appendix G (Links to an external site.). to calculate ΔG°rxn for the following reaction. N2(g) + 3H2(g)<=> NH3(g) Group of answer choices A, -3300J/mol B, 33.0kJ/mol C, -33.0 J/mol D, -33.0kJ/mol
- Calculate the ΔS°rxn of the following reaction at 215°C and standard pressure. C2H4 (g)+302 (g)->2CO2 (g)+2H2 ΔHºf, kJ/mol Sº, J/mol•K ΔGºf, kJ/mol C2H4(g) 52.3 219.5 68.1 O2(g) 0 205.0 0 CO2(g) -393.5 213.6 -394.4 H2O(g) -241.8 188.7 -228.6 _____ J/mol*KWhich energy levels precede and succeed 4s ?Suppose that the gas-phase reaction 2 NO(g) + O2(g)------->2 NO2(g) were carried out in a constant-volume containerat constant temperature. (a) Would the measured heatchange represent ΔH or ΔE? (b) If there is a difference, whichquantity is larger for this reaction? (c) Explain your answer topart (b).
- Consider the reaction CO32-(aq) + H2O(l) HCO3-(aq) + OH–(aq). Kb for CO32- is 2.1 × 10–4 at 25°C. What is Ka for the HCO3- ion at 25°C?For the reaction 2 A --> 2 B + C , Kc = 4.3. If a 2.00 L vessel contains 1.5 mol A,. 2.60 mol B and 3.00 mol C. Determine the value of Qc.I this calculation of the enthalpy of a reaction as measured in a constant pressure telemetry container, I totally get everything except for the exothermic part. I understand that hcl at 25 C mixed with NaOH at 25 degrees gives off h20 and heat, thus exothermic. But what puzzles me is why the formula q = s m delta T yields a positive number indicating an endothermic process. ( final temp higher than initial)
- Urea, CO(NH2)2 is slowly converted to ammonia (NH3) at 25.0 °C according to the following reaction. CO(NH2)2 (aq) + H2O (l) → CO2 (aq) + NH3 (aq) The following data were obtained for this reaction Compound ∆H°f (kJ/mol) CO(NH2)2 (aq) -319.2 H2O (l) -412.9 CO2 (aq) -285.8 NH3 (aq) -80.3 A) Calculate ∆H° for the reaction B) What type of reaction is this (endothermic, exothermic, neither) c)Calculate the change in enthalpy (∆H°) for the decomposition of 2.00 g of urea.From the following reaction and data, find (a) S o of SOCl2 (b) T at which the reaction becomes nonspontaneous SO3(g) + SCl2(l) → SOCl2(l) + SO2(g) Δ G o rxn = −75.2 kJ SO3(g) SCl2(l) SOCl2(l) SO2(g) Δ H o f (kJ/mol) −396 −50.0 −245.6 −296.8 S o (J/mol · K) 256.7 184 − 248.1 S o of SOCl2(l) = J/mol · K T = × 10 K Enter your answer in scientific notation.A+B➡️P t=0 :C(A)=C(B) t=500sec 20% of react t=? Sec 60% of compl