Diatomic iodine [I2] decomposes at high temperature to form I atoms according to the reaction: I2(g)⇌2I(g), Kc=0.011 at 1200∘C In an equilibrium mixture, the concentration of I2 is 0.10 M. What is the equilibrium concentration of I?
Diatomic iodine [I2] decomposes at high temperature to form I atoms according to the reaction: I2(g)⇌2I(g),...
Diatomic iodine (I2) decomposes at high temperature to form I atoms according to the reaction: I2(g)⇌2I(g),Kc=0.011 at 1200∘C In an equilibrium mixture, the concentration of I2 is 0.25 M. What is the equilibrium concentration of I?
The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000 K, the equilibrium constant Kc for the reaction is 3.80 × 10−5. Suppose you start with 0.0458 mol of I2 in a 2.32−L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of I2? __M What is the equilibrium concentration of I? __M
Iodine converts from the molecular form to the atomic form as follows: I2 (g) ⇌ 2I (g) at 500 K. The initial [I2] = 0.45 M and initial [I] = 0. What is [I] at equilibrium? Kc = 5.6 x 10-12 at 500K. Hint: You will need to set up an ICE chart and solve a quadratic equation for this one.
the equilibrium constant for the dissociation of iodine molecules to iodine atoms I2 (g) arrow 2I(g) is 3.76x10^-3 at 1000 K. suppose 0.170 mol of I2 is placed in a 18.7 L flask at 1000 K. what are the concentrations of I2 and I when the system comes to equilibrium?
21.Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000 K, the equilibrium constant Kc for the reaction is 3.80 ×10−5. Suppose you start with 0.0461 mol of I2 in a 2.27−L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of I2? What is the equilibrium concentration of I?
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
Iodine fluoride gas (IF) decomposes to gaseous iodide (I2) and fluoride (F2) at a high temperature. If Kp at this high temperature is 19.7, determine the equilibrium partial pressure of IF gas if its initial concentration was 0.306 atm? Hint: You should write a balanced chemical equation for the reaction described. Question 6 options: 0.153 atm 0.0689 atm 0.168 atm 0.0310 atm 0.138 atm
Iodine fluoride gas (IF) decomposes to gaseous iodide (I2) and fluoride (F2) at a high temperature. If Kp at this high temperature is 19.7, determine the equilibrium partial pressure of IF gas if its initial concentration was 0.306 atm? Hint: You should write a balanced chemical equation for the reaction described. Question 6 options: 0.153 atm 0.0689 atm 0.168 atm 0.0310 atm 0.138 atm
1.The equilibrium constant, Kc, for the reaction of iodine bromide to form iodine and bromine is 2.5*10^-3. If an equilibrium mixture contains 0.58 M IBr and 3.8*10^-2 M I2, what is the molar concentration of Br2? 2IBr(g)—>I2(g)+Br2(g) express answer to two significant figures and include the appropriate units. 2. For the reaction at 225 degrees celsius at the equilibrium contant at 1.7*10^2. If the equilibrium mixture contains 0.24 M H2 and 0.025 M N2, what is the molar concentration of...
Be sure to answer all parts. The equilibrium constant Kc for the reaction I2(g) ⇆ 2I(g) is 3.84 × 10−5 at 724 ° C. Calculate Kc and KP for the equilibrium 2I(g) ⇆ I2(g) at the same temperature. Kc = × 10 (Enter your answer in scientific notation.) KP =