The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products equilibrium. For a gaseous reaction with the general form aA+bB cC + dD the K, and K, expressions are given by K₂ = K₂ = [C] [D] [A] [B] (Pc) (Pb) (PA) (PB) The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved since their composition does not change The standard state of Part A Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl₂(g) = COCk₂2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 460 °C. At equilibrium, the concentrations were measured and the following results obtained: Gas CO Ch₂ COC₂ What is the equilibrium constant, K₂, of this reaction? Express your answer numerically. View Available Hint(s) Partial Pressure (atm) 0.810 1.14 0.270

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Need both parts asap correctly.
The equilibrium constant, K, of a reaction at a
particular temperature is determined by the
concentrations or pressures of the reactants and
products at equilibrium.
For a gaseous reaction with the general form
aA + bB =cC + dD
the K and K, expressions are given by
[C] [D]d
[A] [B]
Kc =
Кр =
(Pc)'(PD)"
(PA)" (PB)
The subscript c or p indicates whether K is
expressed in terms of concentrations or pressures.
Equilibrium-constant expressions do not include a
term for any pure solids or liquids that may be
involved since their composition does not change
throughout the reaction. The standard state of a
pure substance is the pure substance itself, and
although the quantity may change the sample
remain pure. The constant value is incorporated
into the value of K, and does not need to be
accounted for separately.
Part A
Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics.
Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures:
CO(g) + Cl₂ (g) = COC12(g)
Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 460 °C. At equilibrium, the concentrations
were measured and the following results obtained:
What is the equilibrium constant, Kp, of this reaction?
Express your answer numerically.
► View Available Hint(s)
Kp =
Part B
|| ΑΣΦ
K₂ =
Submit
^
P Pearson
Deriving concentrations from data
In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B
however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all
three equilibrium concentrations before you can apply the formula for K.
IVE | ΑΣΦ
Provide Feedback
Gas
CO
Cl₂
|COC1
→
The following reaction was performed in a sealed vessel at 769 °C:
H₂(g) + I2(g) → 2HI(g)
=
Initially, only H₂ and I were present at concentrations of [H₂] = 3.15M and [1₂] = 2.40M. The equilibrium
concentration of I₂ is 0.0300 M. What is the equilibrium constant, Ke, for the reaction at this temperature?
Express your answer numerically.
► View Available Hint(s)
Partial Pressure
(atm)
0.810
1.14
0.270
A
B ?
2 ?
Transcribed Image Text:The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. For a gaseous reaction with the general form aA + bB =cC + dD the K and K, expressions are given by [C] [D]d [A] [B] Kc = Кр = (Pc)'(PD)" (PA)" (PB) The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved since their composition does not change throughout the reaction. The standard state of a pure substance is the pure substance itself, and although the quantity may change the sample remain pure. The constant value is incorporated into the value of K, and does not need to be accounted for separately. Part A Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl₂ (g) = COC12(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 460 °C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp, of this reaction? Express your answer numerically. ► View Available Hint(s) Kp = Part B || ΑΣΦ K₂ = Submit ^ P Pearson Deriving concentrations from data In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K. IVE | ΑΣΦ Provide Feedback Gas CO Cl₂ |COC1 → The following reaction was performed in a sealed vessel at 769 °C: H₂(g) + I2(g) → 2HI(g) = Initially, only H₂ and I were present at concentrations of [H₂] = 3.15M and [1₂] = 2.40M. The equilibrium concentration of I₂ is 0.0300 M. What is the equilibrium constant, Ke, for the reaction at this temperature? Express your answer numerically. ► View Available Hint(s) Partial Pressure (atm) 0.810 1.14 0.270 A B ? 2 ?
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