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, calculate the concentrations of components in the equilibrium mixture at 425 oC.
Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and...
4.00 mols of H2 and 3 mols of I2 are placed in an evacuated 5.00L flask and then heated to 800K. The system is allowed to reach equilibrium. what will be the equilibrium concentration of each species? 2HI(g) <-----> H2(g) + I2(g) Kc= 0.016 @ 800k
Consider the equilibrium reaction. H2(g) + I2(g) equilibrium reaction arrow 2 HI(g) In this case, 1.000 M H2 reacts with 2.000 M of I2 at a temperature of 414°C. The value of Kc = 72. Determine the equilibrium concentrations of H2, I2, and HI. [H2] [I2] [HI]
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?
2.50 mole of diatomic astatine is placed in a 1.0 L flask with 0.900 mole of fluorine gas and the flask is stoppered. When the mixture comes to equilibrium, the concentration of monoastatine monofluoride is 1.19 M. What is the equilibrium constant for this reaction? Please show all work including an ICE table Thank you for your time
For the reaction H2 (g) + I2 (g) = 2HI (g); Kc =50.0. Calculate the concentration of HI (g) at equilibrium if the initial concentration of each substance is 0.0600 M and the reaction mixture is allowed to come to equilibrium. (Hint: ICE Table)
H2(g)+I2(g)⇌2HI(g) For the above reaction, Kc=55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.053 g of H2 and 4.39 g of I2. What is the mass of HI in the flask?
Kc for the reaction of hydrogen and iodine to produce hydrogen iodide, H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Determine the initial and equilibrium concentration of HI if initial concentrations of H2 and I2 are both 0.10 M and their equilibrium concentrations are both 0.052 M at 430°C
Hydrogen gas, iodine vapor, hydrogen iodine are mixed in a flask and heated to 642°C. H2(g) + I2(g) ⇋ 2 HI(g) Kc = 53 at 642°C If the initial concentrations of hydrogen gas and iodine vapor are both 0.054 mol/L and the concentration of hydrogen iodine is 0.130 mol/L what is the equilibrium concentration of hydrogen gas? Enter a number to 4 decimal places.
Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.200 M and [I2] = 0.400 M. The equilibrium constant Kc for the reaction following reaction is 57.0 at 700 K. (Show Work) H2(g)+I2(g)<--- ---->2HI(g)
For the reaction H2(g)+I2(g)⇌2HI(g), Kc= 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.053 g H2 and 4.38 g I2. What is the mass of HI in the flask? Express your answer to two significant figures and include the appropriate units.