The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000...
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?
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Homework Answers
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The dissociation of molecular iodine into iodine atoms is
represented as
I2(g) ⇌ 2I(g)
At 1000...
21.Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented...
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?
the equilibrium constant for the dissociation of iodine molecules to iodine atoms I2 (g) arrow 2I(g)...
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?
Please help me with this question and help me understand that. Be sure to answer all...
Please help me with this question and help me understand
that.
Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as I2(g) - 21g) 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 2.33-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...
3 attempts left Check my work Be sure to answer all parts. The dissociation of molecular...
3 attempts left Check my work Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as 126) = 2(g) At 1000 K, the equilibrium constant K for the reaction is 3.80 x 10 . Suppose you start with 0.0451 mol of I, in a 2.33-L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of IZ? M What is the equilibrium concentration of I?...
Be sure to answer all parts. The dissociation of molecular lodir Is represented as 13C) =...
Be sure to answer all parts. The dissociation of molecular lodir Is represented as 13C) = 2(g) brium constant for the reaction is 3.80 X 10. Suppose you start with 0.0454 mol of 1 in a 2.33-L flask the concentrations of the gases at equilibrium? Wha the equilibrium concentration of 1,? What is the equilibrium concentration of I?
1)Consider the following equilibrium at 972 K for the dissociation of molecular iodine into atoms of...
1)Consider the following equilibrium at 972 K for the dissociation of molecular iodine into atoms of iodine. I2(g) ----> 2 I(g); Kc = 1.40 ? 10?3 Suppose this reaction is initiated in a 3.4 L container with 0.067 mol I2 at 972 K. Calculate the concentrations of I2 and I at equilibrium. * I got I2= 0.0135M and I= 0.0124 is this right?* 2)Consider the following equilibrium. NH3(aq) + H2O(l) -----> NH4+(aq) + OH ?(aq) What will happen to the...
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 0.10 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),Kc=0.011...
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?
Iodine converts from the molecular form to the atomic form as follows: I2 (g) ⇌ 2I...
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.
Molecular iodine, I2 (g), dissociates into iodine atoms at 652 K, with a first order rate...
Molecular iodine, I2 (g), dissociates into iodine
atoms at 652 K, with a first order rate constant of 0.452
s-1.
a. What is the half life for this reaction?
[ Select ]
["1.53 s", "0.31 s", "0.079 s", "0.39 s"]
b. If you start with 0.35 M I2 at this temperature,
how long will it take for the concentration of I2 to
reach...
Please help me with this question and help me understand
that.
Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as I2(g) - 21g) 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 2.33-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...
3 attempts left Check my work Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as 126) = 2(g) At 1000 K, the equilibrium constant K for the reaction is 3.80 x 10 . Suppose you start with 0.0451 mol of I, in a 2.33-L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of IZ? M What is the equilibrium concentration of I?...
Be sure to answer all parts. The dissociation of molecular lodir Is represented as 13C) = 2(g) brium constant for the reaction is 3.80 X 10. Suppose you start with 0.0454 mol of 1 in a 2.33-L flask the concentrations of the gases at equilibrium? Wha the equilibrium concentration of 1,? What is the equilibrium concentration of I?
Molecular iodine, I2 (g), dissociates into iodine
atoms at 652 K, with a first order rate constant of 0.452
s-1.
a. What is the half life for this reaction?
[ Select ]
["1.53 s", "0.31 s", "0.079 s", "0.39 s"]
b. If you start with 0.35 M I2 at this temperature,
how long will it take for the concentration of I2 to
reach...
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