1. In the upper atmosphere, ozone is produced from oxygen gas in the following reaction.
3O2(g) → 2O3(g)
Calculate ΔGo for this reaction. (Enter your answer in kJ and give 3 significant figures.)
2. Calculate ΔHo for ozone formation. (Enter your answer in kJ and give 3 significant figures).
3. Calculate ΔSo for ozone formation. (Enter your answer in J/K and give 3 significant figures).
4. Assume an atmosphere where p(O2) = 0.080 atm, and where T = 298 K. Below what pressure of O3 will ozone production be spontaneous? (Enter your answer in atm).
1. In the upper atmosphere, ozone is produced from oxygen gas in the following reaction. 3O2(g)...
In the upper atmosphere, ozone is produced from oxygen gas in the following reaction. 3O2(g) → 2O3(g) Calculate ΔGo for this reaction. Enter your answer in kJ and give 3 significant figures. Calculate ΔHo for ozone formation. (Enter your answer in kJ and give 3 significant figures). Calculate ΔSo for ozone formation. (Enter your answer in J/K and give 3 significant figures). Assume an atmosphere where p(O2) = 0.120 atm, and where T = 298 K. Below what pressure of...
ozone can be created from oxygen gas (with an input of energy) via the following reaction: 3O2(g)=2O3(g) If the equilibrium constant, K, is 1.12 * 10^-54 for this reaction at a particular temperature and [O2]= 3.10*10^-2 M at equilibrium, what is [O3] (in M to two decimal places) at equilibrium? Ans: 5.78 * 10^-30 M
For the reaction: 2NO(g) + O2(g) ----> 2 NO2(g) ΔGo = −67.3 kJ and ΔSo= 146.5 J/K at 345K and 1 atm. Calculate the standard enthalpy change for the reaction of 3.75 moles of NO(g) at this temperature.Use 4 sig. figures. Hint: The ΔHo (heat absorbed or released) you have calculated is when 2 moles of NO reacted.
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. b. Determine the temperature(oC) at which the reaction is at equilibrium.
Calculate deltaG at 298K for the formation of one mole of ozone, O3, from oxygen gas, O2, when [O2]= 0.210 atm and [O3]= 5.00 x 10-7 atm. 3/2 O2 (g) ---> O3 (g) deltaHo= 143Kj, deltaSo= -.06868kJ/K the answer is 133 kJ/mol
Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) --> NO2(g) + O2(g). ( ΔH° = –199 kJ/mol, ΔS° = –4.1 J/K·mol) Write answers to three significant figures. a. Calculate the ΔG°( kJ/mol) for this reaction at 25°C. Blank 1 b. Determine the temperature(oC) at which the reaction is at equilibrium.
Ozone (O3) in the atmosphere can be converted to oxygen gas by reaction with nitric oxide (NO). Nitrogen dioxide is also produced in the reaction. What is the enthalpy change when 8.50L of ozone at a pressure of 1.00 atm and 25°C reacts with 12.00 L of nitric oxide at the same initial pressure and temperature? [∆H°f (NO) = 90.4 kJ/mol; [∆H°f (NO2) = 33.85 kJ/mol; ∆H°f (O3)= 142.2 kJ/mol] [O3 + NO O2 + NO2] show all work...
Ozone (O3) in the atmosphere can react with nitric oxide (NO): 03(g) + NO(g) --> NO2(g) + O2(g). (AH° = -199 kJ/mol, 45º = -4.1 J/K·mol) Write answers to three significant figures. a. Calculate the AG°(K9/02.) for this reaction at 25°C. b. Determine the temperature(°C) at which the reaction is at equilibrium.
For the following reaction: 3O2(g) ------> 2O3(g) delta H= 285.4kJ Will the reaction be spontaneous, nonspontaneous, or impossible to determine at standard conditions. Briefly explain your answer.
2-Consider the reaction H2(g) + Br2(g) 2 HBr (g⇌ ) where ΔHo = -36.4 kJ/mol. In one experiment, equal amounts in moles of H2(g) and Br2(g) were mixed in a 2.00 L chamber at 25 oC exerting a pressure P = 1.0 atm. After mixture reached equilibrium, partial pressure of H2 gas PH2 was measured using high sensitivity HVAC gauge recording, PH2 = 5x10-4 Pa. For this equilibrium reaction, answer the following: (i)Calculate the total amount nT of gases...