For the following reaction, K is 910 when temperature (T) is 800K; K is 1 when temperature (T) is 1050K. Calculate ΔrHm ○
2SO2 (g)+O2 (g) →2SO3 (g)
For the following reaction, K is 910 when temperature (T) is 800K; K is 1 when...
The equilibrium constant, Kc, for the following reaction is 5.63×10-2 at 1190 K. 2SO3(g) 2SO2(g) + O2(g) Calculate Kc at this temperature for: 2SO2(g) + O2(g) 2SO3(g)
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
A student ran the following reaction in the laboratory at 1078 K: 2SO3(g)-> 2SO2(g) + O2(g) When she introduced 7.35×10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 1.53×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
1- The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) --------> H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.395 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [I2] = M 2- student ran the following reaction in the laboratory at 1090 K: 2SO3(g) ----------> 2SO2(g) + O2(g) When he introduced SO3(g) at a pressure of 1.05 atm into a 1.00...
A student ran the following reaction in the laboratory at 1185 K: 2SO2(g) + O2(g) 2SO3(g) When she introduced 8.07×10-2 moles of SO2(g) and 7.94×10-2 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of O2(g) to be 5.86×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1270 K? Kp =
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1260 K? Kp= ?
If the equilibrium constant for reaction X is K. What is the equilibrium constant for reaction Y is? Reaction X: SO2 (g) + (1/2) O2 (g) ⇌ SO3 (g) Reaction Y: 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) a. 2K b. K2 c. 1/K2 d. 0.5 x K e. -K2
A reaction vessel at 1215 K contains a mixture of SO2(P= 3.10 bar ) and O2(P= 1.20 bar ). When a catalyst is added the reaction 2SO2(g)+O2(g)⇌2SO3(g) takes place. At equilibrium the total pressure is 4.05 bar .
for the reaction: 2SO2(G)+O2(G)--->2SO3(G)+197kJ show graphically how the equilibrium system will respond to what happens when temperature is decreased.