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 a given reaction, ΔrH = +35.5 kJ mol-1 and ΔrS = +83.6 J K-1 mol-1. The reaction is spontaneous ________. Assume that ΔrH and ΔrS do not vary with temperature. A. at all temperatures B. at T < 298 K C. at T < 425 K D. at T > 425 K E. at T > 298 K
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
1 What is the equilibrium constant for a reaction at temperature 89.1 °C if the equilibrium constant at 22.6 °C is 49.93? For this reaction, ΔrH = -21.1 kJ mol-1 . 2 What is the ΔrG° for the following reaction (in kJ mol-1)? C6H12O6(s, glucose) + 6 O2 (g) ⇌6 CO2 (g)+ 6 H2O (l) 3 What is the ΔrG° for the following reaction (in kJ mol-1)? 2 NO2 (g) ⇌N2O4 (g) 4 What is the ΔrG for the following...
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...