For the reaction: SO2(g) + ½ O2(g) = SO3(g) , Keq= 6.55 at 900K and Keq=...

Question

Question

For the reaction:

SO₂(g) + ½ O₂(g) = SO₃(g) , K_eq= 6.55 at 900K and K_eq= 1.86 at 1000 K

Calculate Δ_rH° over the temperature range 900 K - 1000 K (assume Δ_rH° is constant)

Answer 1

Answer #1

We have, T1 = 900 K K 6.55 2- 1000 K K, = 1.86 According to VantHoff equation, 1.86 6.558.314 JKmol900 K 1000 ΔΗ。 AHng (0.000

Answer 2

Similar Homework Help Questions

Calculate Δ G for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g)...

Calculate Δ G for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) when P of SO2 = 0.500 atm, P of O2 = 0.0100 atm, and P of SO3 = 0.100 atm. The value for Δ G^o for this reaction at 298 K is -141.6 kJ. ΔG = ???? kJ I got -160.9 kj but it is incorrect.
Calculate AG for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) when...

Calculate AG for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) when P of SO2 = 0.500 atm, P of O2 = 0.0100 atm, and P of SO3 = 0.100 atm. The value for AGº for this reaction at 298 K is -141.6 kJ. AG= O * kJ Is this reaction spontaneous or non-spontaneous under these conditions? Spontaneous or non-spontaneous? spontaneous
The equilibrium constant for the following reaction is 1.71×10-2 at 847 °C. 2 SO3(g)2 SO2(g) +...

The equilibrium constant for the following reaction is 1.71×10-2 at 847 °C. 2 SO3(g)2 SO2(g) + O2(g) K = 1.71×10-2 at 847 °C Calculate the equilibrium constant for the following reactions at 847 °C. (a) 2 SO2(g) + O2(g)2 SO3(g) K = (b) SO3(g) SO2(g) + 1/2 O2(g) K = Show Approach

For the reaction 2 SO2(g) + O2(g) →→2 SO3(g) AG° = -140.3 kJ and AS =...

For the reaction 2 SO2(g) + O2(g) →→2 SO3(g) AG° = -140.3 kJ and AS = -187.9 J/K at 306 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 306 K. The standard enthalpy change for the reaction of 1.79 moles of so,(g) at this temperature would be
Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above...

Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above reaction is allowed to reach equilibrium prior to the following changes. Answer the following questions by writing increase, decrease or remain the same on the line. **please also explain why** If the reaction mixture is heated up , the value of the equilibrium constant will _______________________ If SO2 (g) is added to the reaction vessel the concentration of O2(g) will____________________________. If SO3 (g) is...
3. Consider the following reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (g) AH.x...

3. Consider the following reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (g) AH.x = -197.6 kJ a. If 285.3 g of SO2 is allowed to react with 158.9 g of O2, what is the limiting reactant and theoretical yield of SO3 in liters if the reaction is performed at 315 K and 50.0 mmHg? How much of each reactant remains at the end of the reaction? [10] LR: SO TY: SO2 remaining: O2 remaining: Imol soa 64.000log...

5) For the reaction 2 SO2(g) + O2(g) → 2 SO3(g), if initially P(SO2) = 1.2...

5) For the reaction 2 SO2(g) + O2(g) → 2 SO3(g), if initially P(SO2) = 1.2 atm, P(O2) = 1.8 atm, and P(SO3) = 2.1 atm, calculate AG for this reaction at 25°C. The following data is valid at 25°C: AG° (kJ/mol) SO 300.4 SO3 370.4 A) -140.0 kJ/mol B)-141.3 kJ/mol C)-138.7 kJ/mol D) 1,174.7 kJ/mol E) -137.6 kJ/mol
The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8...

The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8 x 103 Which direction will the reaction proceed if [502] = 0.015 M. [02] = 0.010 Mand (SO3) = 0.200 M? no shift shifts to make more product shifts to make more reactant
For the equilibrium 2 SO3(g) <----> 2 SO2(g) + O2(g), Kc is 4.08 * 10-3 at...

For the equilibrium 2 SO3(g) <----> 2 SO2(g) + O2(g), Kc is 4.08 * 10-3 at 1000 K. Calculate the value for Kp.

A) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g)...

a) An important reaction in the manufacture of sulfuric acid is the oxidation of SO2(g) to SO3(g): 2. 2SO2(g) O2(g)SO3(g) dGo, ΔΗο, and ASo values for the reaction are-141 .6kJ/mol,-1984kJ/mol and -187.9J/Kmol, respectively. Evaluate whether or not the reaction is spontaneous under standard conditions at 298K, predict the effect of increasing temperature on spontaneity and calculate the value of T at which the reaction becomes nonspontaneous. b) The reaction described in part (a) is too slow at room temperature to...