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40. Consider the following reaction equation: SO2 + NO2 → SO3+NO If.35 moles of SO2 and...
For the chemical equation SO2(g)+NO2(g)↽−−⇀SO3(g)+NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.20 mol SO2(g) in order to form 1.00 mol SO3(g) at equilibrium. moles of NO2(g):
For the chemical equation SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) the equilibrium constant at a certain temperature is 2.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 3.36 mol SO2(g) in order to form 1.40 mol SO3(g) at equilibrium.
At 550 K, the reaction- SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) has Kc = 770. If 0.496 moles of SO3 and 0.496 moles of NO are placed in a 5.00-L container at 550 K, what is the concentration of SO3 at equilibrium? A) 4.3 M B) 0.096 M C) 0.099 M D) 17 M E) 0.025 M
Consider the following reaction and its equilibrium constant: SO2(g) + NO2(8) - SO3(g) + NO(g) Kc=0.33 A reaction mixture contains 1.0 mol L-1 SO2, 0.50 mol L-1 NO2,0.50 mol L-1 SO3, and 1.0 mol L-1 NO. Which of the following statements is TRUE concerning this system? A) The reaction will shift in the direction of reactants. B) The system is at equilibrium. C) The reaction quotient will decrease. D) The reaction will shift in the direction of products. E) The...
1. At a particular temperature, K = 2.50 for the reaction: SO2 (g) + NO2 (g) ⇄ SO3 (g) + NO (g). If all four gases had initial concentrations of 1.00 M, calculate the equilibrium concentrations of SO2. 2. At a particular temperature, Kp = 0.25 for the reaction: N2O4 (g) ⇄ 2 NO2 (g). A flask containing only N2O4 at an initial pressure of 4.5 atm is allowed to reach equilibrium. a. Calculate the equilibrium partial pressure of N2O4....
27. Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = SO3(g) + NO(g) Kc = 0.33 A reaction mixture contains 0.41 M SO2, 0.13 M NO2.0.11 M SO3 and 0.13 M NO. Which of the following statements is TRUE concerning this system? A) The reaction will shift in the direction of reactants. B) The equilibrium constant will decrease. C) The reaction will shift in the direction of products. D) The reaction quotient will decrease. E) The system...
The reaction NO2(g) + SO2(g) ⇌NO (g) + SO3(g) has a Kc =10 under some conditions. If the initial concentrations of both NO2 and SO2 are 0.5 M, then calculate the equilibrium concentrations of all four species. [NO2]eq= __________ [SO2]eq= __________ [NO]eq= __________ [SO3]eq= _________
At a particular temperature, K = 3.75 for the reaction: SO2(g) + NO2(g) SO3(g) + NO(g). If all four gases had initial concentrations of 0.250 M, calculate the equilibrium concentrations of the gases.
For the chemical equation SO2(g) + NO2(g) – SO2(g) + NO(g) the equilibrium constant at a certain temperature is 2.00. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.31 mol SO2(g) in order to form 1.10 mol SO3(g) at equilibrium. moles of NO2(g): _______ mol
13. Consider the following When 0.600 moles of SO and allowed to reach equi Keq value. 13. Consider the following equilibrium: 2 SO2(g) + O2(g) +2 SO3 (8) smo ) Set up your ICE table When 0.600 moles of SO2 and 0.600 moles of O2 are placed into a 1.00-liter container and allowed to reach equilibrium, the equilibrium (SO3) becomes 0.250 M. Calculate the Keq value = (0.83 a) Set up your ICE table 0.60 Ans: ve for keq. b)...