Lightning bolts have been found to enable the following
atmospheric reaction:
?2 +?2 →2?? ?r ?°=175.2?????−1 ?? 298?
a) The ΔrH° of this reaction is 182.6 kJ mol-1 and the ΔrS° is 24.8 J mol-1 K-1. Calculate the temperature at which this reaction changes between being spontaneous to non-spontaneous. Report your answer in K. Show your work.
b) Using the reaction above, along with the knowledge that ∆??° (??2 (?) = 51.3 ?? ???−1 at 298 K, calculate ΔrG° (in kJ mol-1) for the following reaction at 298 K. Show your work.
??2(?) + ??(?) → ?2(?) + 3/2 ?2(?)
Lightning bolts have been found to enable the following atmospheric reaction: ?2 +?2 →2?? ?r ?°=175.2?????−1...
6. Lightning bolts have been found to enable the following atmospheric reaction: N26) + O2(g) → 2 NO(g) 4,Gº = 175.2 kJ mol-1 at 298 K a) (2 marks) The AH of this reaction is 182.6 kJ mol- and the A.Sº is 24.8J molK1. Calculate the temperature at which this reaction changes between being spontaneous to non-spontaneous. Report your answer in K. Show your work b) (3 marks) Using the reaction above, along with the knowledge that A,Gº (NO2 )...
For the decomposition of barium carbonate, consider the following thermodynamic data: ΔrH∘ΔrH∘ 271.5kJ mol−1 ΔrS∘ΔrS∘ 173.8J K−1 mol−1 A: Calculate the temperature in kelvins above which this reaction is spontaneous. Answer:1562K B: Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C: BaCO3(s)→BaO(s)+CO2(g) Answer: 2.73*10^-39 C: When adjusted for any changes in ΔrH and ΔrS with temperature, ΔrG∘(600K)=167kJ mol−1. Calculate the equilibrium constant at 600 K .
What is ΔrH for a reaction that has ΔrG = -26.3 kJ mol-1 and ΔrS = 44.9 J mol-1 K-1 at -9.0 °C? Express your answer in kJ mol-1.
What is ΔrG for a reaction that has ΔrH = 86.7 kJ mol-1 and ΔrS = 83.7 J mol-1 K-1 at 3.3 °C? Express your answer in kJ mol-1 .
What is ΔrH for a reaction that has ΔrG = -0.2 kJ mol-1 and ΔrS = 65.4 J mol-1 K-1 at 48.2 °C? Express your answer in kJ mol-1 .
Consider the following reaction: 4??2(?) +?2(?) +2?2?(?) →4???3(?) ΔrG° = -70.8 kJ mol-1 at 298 K, and ΔrH° = -346 kJ mol-1 a) What is the equilibrium constant at 298 K? b) At what temperature (in K) will K = 1? just need help with B PLEASE
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The chemical reaction that causes iron to corrode in air is given by 4Fe(s)+3O2(g)→2Fe2O3(s) 4 F e ( s ) + 3 O 2 ( g ) → 2 F e 2 O 3 ( s ) and ΔrH∘ Δ r H ∘ = −1684 kJ mol−1 = − 1684 k J m o l − 1 ΔrS∘ Δ r S ∘ = −543.7 J K−1 mol−1 = − 543.7 J K − 1 m o l − 1 part...
For the following reaction and data: 1 2 ?2 (?) + ?2 (?) ⇌ ??2 (?) ∆??° = 33.2 ?? ??? −1 ∆??° = −60.9 ? ??? −1? −1 ?° (?2 (?)) = 191.6 ? ??? −1? −1 ?°(??2 (?)) = 240.1 ? ??? −1? −1 a) What is S° for O2 (g) ? b) At standard state conditions, which of the following statements is true about the reaction as written? - Spontaneous at all temperatures - Spontaneous at low...
1.A) What is the equilibrium constant for a reaction at temperature 31.5 °C if the equilibrium constant at 55.4 °C is 1.53? For this reaction, ΔrH = 20.2 kJ mol-1 . You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". 1B) What is the ΔrG° for the following reaction (in kJ mol-1)? N2(g) + O2(g) + Cl2(g)...