1mol of H2, 2.0mol of I2, 3mol of HI are injected into 1 Litre flask. What will be the equilibrium concentration of H2, I2, HI at 490^C? The equilibrium constant for the reaction is 45.9.
1mol of H2, 2.0mol of I2, 3mol of HI are injected into 1 Litre flask. What...
The following reaction was performed in a sealed flask at 999 degreesCelsius. H2 (g) + I2 (g) 2 HI (g) Kc = 222. If H2 and I2 are both 0.15 M at equilibrium, what is the concentration of HI at equilibrium?
Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and the mixture is heated to 425oC. At equilibrium, the concentration of I2 is found to be 0.0210 M. a) What are the equilibrium concentrations of H2 and HI, respectively? Calculate Kc for the following reaction at 425oC. H2(g) + I2(g) ⇄ 2 HI(g) b) If the initial concentrations of H2 and I2 are 1.000 M each, and the initial concentration of HI is 0.000,...
An equilibrium mixture contains 0.950 mol HI, 0.490 mol I2, and 0.290 mol H2 in a 1.00-L flask. What is the equilibrium constant for the following reaction? 2HI(g) H2(g) + I2(g) K = How many moles of I2 must be removed in order to double the number of moles of H2 at equilibrium? mol I2
consider the equilibrium reaction of H2 (g) + I2 (g) <-----> 2 HI (g) it has an equilibrium constant Kc = 54.3 at 430°C. if the initial concentration of [HI]0 = 2.000 M. what are the equilibrium concentrations?
The following reaction: H2 (g) + I2 (g) ⇋ 2 HI (g) Has an equilibrium constant of 30.5 under certain conditions. If initial concentrations of reactants and product are: [H2] = 0.100 M; [I2] = 0.100 M; and [HI] = 0.250 M, what will be the equilibrium concentration of HI?
Given the reaction below, H2 (g)+ I2 (g)⇌ 2 HI (g) Kc = 50.5 What was the initial mass of HI (g) placed in a sealed 1.50 L flask which resulted in 0.025 mol of each of H2 (g) and I2 (g) being found in the flask at equilibrium?
Suppose a 250.mL flask is filled with 1.9mol of H2 and 1.7mol of I2. The following reaction becomes possible: H2(g) + I2(g) 2HI(g) The equilibrium constant K for this reaction is 5.99 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.
At 6 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI, H2, and I2? We were unable to transcribe this imageAt 6 °C the equilibrium constant for the reaction: 2 HI(g) = H2(g) + 12(g) is Kp = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI,...
1/2 H2 (g) + 1/2 I2 (g) <-> HI (g) At a certain temperature, Kc of reaction is 400 If 0.025M of H2 and 0.025 M and 0.065 M of HI are in a 1.00 L container, what is the concentration of HI at equilibrium?
At 49 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP = 4.83e-11. If the initial pressure of HI is 0.00862 atm, what are the equilibrium partial pressures of HI, H2, and I2? p(HI) = p(H2) = . p(I2) = .