The following reaction can occur at 298K under appropriate conditions. 2SO2(g) +O2(g)-----> 2SO3(g) An equilibrium mixture...

The following reaction can occur at 298K under appropriate conditions.
2SO2(g) +O2(g)-----> 2SO3(g)
An equilibrium mixture contain O2(g) and SO3(g) at partial pressure of 0.50atm and 2.0atm respectively. Using data available in Appendix 4 of your textbook, determine the equilibrium partial pressure of SO2 in the mixture. Will this reaction be most favored at a high or at a low temperature, assuming standard conditions? Justify your reasoning
Substance.             delta H°              S°
SO2(g)                     -297.                    248
SO3(g)                     -396.                     257
O2(g)                         0.                         205

Expert Solution

Please upvote!

queen_honey_blossom answered 1 year ago

Consider the following reaction at 388 K 2SO2 (g) + O2 (g) <==> 2SO3 (g) At...

Consider the following reaction at 388 K 2SO2 (g) + O2 (g) <==> 2SO3 (g) At equilibrium the reaction mixture contains 1.28 atm of O2 and 6.78 atm of SO3. The equilibrium constant, KP, at this temperature is 46.7. Calculate the equilibrium partial pressure of SO2.

The following reaction wax examined at 250 C 2SO3(g) <--------- -------------> 2SO2(g) + O2(g) At a...

The following reaction wax examined at 250 C 2SO3(g) <--------- -------------> 2SO2(g) + O2(g) At a particular temperature , 14.5 mole SO3 is placed in to a 2.0 L container and dissociates according to the reaction above. At equilibrium 3.0 mole of SO2 is present. Calculate Kc for this reaction

-A student ran the following reaction in the laboratory at 1143 K: 2SO2(g) + O2(g) 2SO3(g)...

-A student ran the following reaction in the laboratory at 1143 K: 2SO2(g) + O2(g) 2SO3(g) When she introduced 8.19×10-2 moles of SO2(g) and 8.56×10-2 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 6.08×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =____________ -A student ran the following reaction in the laboratory at 363 K: CH4(g) + CCl4(g) 2CH2Cl2(g) When she introduced 4.64×10-2 moles of CH4(g) and...

For the reaction 2SO2(g) + O2(g) → 2SO3(g), ΔH° and ΔS° are both negative at 298...

For the reaction 2SO2(g) + O2(g) → 2SO3(g), ΔH° and ΔS° are both negative at 298 K, and the process is spontaneous at 298 K. Which of the following statements must also be true? A.ΔG is positive for the reaction at 298 K. B.The change in entropy is the driving force of the reaction. C.ΔG is temperature independent. D.The direction of the reaction may be reversed at high temperatures. E.At high temperature, ΔH becomes positive.

For 2SO2(g)+O2(g)⇌2SO3(g), Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.13 g...

For 2SO2(g)+O2(g)⇌2SO3(g), Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.13 g of SO3 and 0.104 g of O2 How many grams of SO2 are in the vessel?

2SO2(g) + O2(g) <--> 2SO3(g) A sealed reaction vessel is charged with 5.0 atm SO2 and...

2SO2(g) + O2(g) <--> 2SO3(g) A sealed reaction vessel is charged with 5.0 atm SO2 and 2.5 M atm at 500 degrees Celsius. The reaction is allowed to equilibriate. At equilibrium 3.0 atm of SO3 is produced. What is the equilibrium concentration of each species. What is Kc for this reaction? Show all work.

Given the following equilibrium system: 2SO2(g) + O2(g) ↔ 2SO3(g) + 99.1 kJ If additional SO2(g)...

Given the following equilibrium system: 2SO2(g) + O2(g) ↔ 2SO3(g) + 99.1 kJ If additional SO2(g) is added to the system while the temperature and pressure are kept constant. Compared to its original concentration, how will the concentration, of oxygen change? Increase Decrease Remain the Same The pressure on the system is increased while the temperature is kept constant. Compared to its original concentration, how will the concentration of SO2(g) change? Decrease Increase Remain the Same A catalyst is added...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part A If 276.0 mL of SO2 is allowed to react...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part A If 276.0 mL of SO2 is allowed to react with 161.4 mL of O2 (both measured at 327 K and 48.7 mmHg ), what is the limiting reactant? Part B What is the theoretical yield of SO3? nSO3 = Part C If 175.8 mL of SO3 is collected (measured at 327 K and 48.7 mmHg ), what is the percent yield for the reaction? Express your answer using four significant figures.

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) What is the theoretical yield of SO3? If 188.5 mL of...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) What is the theoretical yield of SO3? If 188.5 mL of SO3 is collected (measured at 327 K and 54.5 mmHg ), what is the percent yield for the reaction?

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part B What is the theoretical yield of SO3? nSO3 =...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part B What is the theoretical yield of SO3? nSO3 = Part C If 175.8 mL of SO3 is collected (measured at 327 K and 48.7 mmHg ), what is the percent yield for the reaction? Express your answer using four significant figures.

Question