What must be true of the exponents of the rate law for the reaction 2So2(g)+O2(g)--> 2SO3(g) when the rate law is expressed as rate=k[SO2(g)]^x[O2(g)]^y
What must be true of the exponents of the rate law for the reaction 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)
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at a certain temperature. If at equilibrium, [SO2] = 0.0451 M and [O2] = 0.078 M, what is the equilibrium [SO3]?
Consider the reaction: 2SO2(g)+O2(g)→2SO3(g) a) If 287.8 mL of SO2 reacts with 166.6 mL of O2 (both measured at 323 K and 67 mbar ), what is the limiting reactant? b) What is the theoretical yield of SO3? c) If 180.2 mL of SO3 is collected (measured at 323 K and 67 mbar ), what is the percent yield for the reaction?
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=?
Consider the following reaction where Kc = 34.5 at 1150 K: 2SO2(g) + O2(g) =2SO3(g) A reaction mixture was found to contain 4.39x10-2 moles of SO2(g), 4.28x10-2 moles of O2(g) and 4.23x10-2 moles of SO3(), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium SO3(g) must be consumed. 2. In order to reach equilibrium Kc must decrease. 3. In order to reach equilibrium SO2 must be consumed....
Consider the reaction: 2SO2(g) + O2(g)2SO3(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.11 moles of SO2(g) react at standard conditions. S°system = J/K
Consider the reaction 2SO2(g) + O2(g)2SO3(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.11 moles of SO2(g) react at standard conditions. S°surroundings = J/K
At 900 K the following reaction has Kp=0.345: 2SO2(g)+O2(g)???2SO3(g) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.150atm and 0.465atm , respectively. What is the equilibrium partial pressure of SO3 in the mixture?
Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) If 274.2 mL of SO2 is allowed to react with 159.0 mL of O2 (both measured at 322 K and 54.4 mmHg Part A: What is the theoretical yield of SO3? Part B: If 180.2 mL of SO3 is collected (measured at 322 K and 54.4 mmHg ), what is the percent yield for the reaction?
Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) If 285.0 mL of SO2 is allowed to react with 163.8 mL of O2 (both measured at 324 K and 54.7 mmHg ), what is the limiting reactant? B.What is the theoretical yield of SO3? C.If 188.0 mL of SO3 is collected (measured at 324 K and 54.7 mmHg ), what is the percent yield for the reaction? Express your answer using four significant figures.