The equilibrium concentrations in a gas mixture at a particular temperature are 0.13 M H2, 0.70...
The equilibrium concentrations in a gas mixture at a particular temperature are 0.13 M H2, 0.70 M I2, and 2.1 HI.
What equilibrium concentrations are obtained at the same temperature when 0.19 mol of HI is injected into an empty 460 mL container?
Express your answer using two significant figures. Enter your answers numerically separated by commas.
Homework Answers
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The equilibrium concentrations in a gas mixture at a particular
temperature are 0.13 M H2, 0.70...
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2...
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2 and 2.35 mol of I2 are placed in a 10.0 L flask and allowed to come to equilibrium, at which time 3.76 mol of HI are present. The reaction is H2(g) + I2(g) --> 2HI (g) What is the value of Kc? What is the value of Kp?
Consider the following equilibrium with a Kc = 55.6 at a temperature of 698 K. H2(g)...
Consider the following equilibrium with a Kc = 55.6 at a temperature of 698 K. H2(g) + I2(g) <--> 2HI(g) ΔH0 = + 26.5 kJ / mol If the initial concentrations were [H2] = 0.12 M; [I2] = 0.041 M; and [HI] = 2.6 M. Is the system at equilibrium, and if not, in which direction must it shift to establish equilibrium? Justify your answer. At the same 698 K, 0.50 mol of H2 and 0.88 mol of I2 are...
The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations...
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 Kc and Kp expressions are given by Kc=[C]c[D]d[A]a[B]b Kp=(PC)c(PD)d(PA)a(PB)b 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...
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2...
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2 and 2.35 mol of I2 are placed in a 10.0 L flask and allowed to come to equilibrium, at which time 3.76 mol of HI are present. The reaction is b) What is the value of Kc? c) What is the value of Kp
At a particular temperature, K = 7.40 × 102 for the reaction H2 (g) + 12...
At a particular temperature, K = 7.40 × 102 for the reaction H2 (g) + 12 (g) 늑 2H1(g) In an experiment, 3.30 moles of H2, 3.30 moles of I2, and 3.30 moles of HI are introduced into a 1.00-L container Calculate the concentrations of all species when equilibrium is reached Concentration of H2 = Concentration of - Concentration ofHi-M
Equilibrium Concentrations -- A + B = 2C At a particular temperature, K = 1.00×102 for...
Equilibrium Concentrations -- A + B = 2C
At a particular temperature, K = 1.00×102
for the reaction:
H2(g) + F2(g)
2HF(g)
In an experiment, at this temperature, 1.00×10-1 mol
of H2 and 1.00×10-1 mol of F2 are
introduced into a 1.09-L flask and allowed to react. At
equilibrium, all species remain in the gas phase.
What is the equilibrium concentration (in mol/L) of
H2?
mol/L
1 pts
What is the equilibrium concentration (in mol/L) of HF?
mol/L
1 pts...
For the reaction below at a certain temperature, it is found that the equilibrium concentrations in...
For the reaction below at a certain temperature, it is found
that the equilibrium concentrations in a 5.05-L rigid container are
[H2] = 0.0523 M, [F2] = 0.0121
M, and [HF] = 0.450 M.
H2(g) + F2(g) 2
HF(g)
If 0.203 mol of F2 is added to this equilibrium
mixture, calculate the concentrations of all gases once equilibrium
is reestablished.
An equilibrium mixture of H2, I2, and HI at 458 ∘C contains 0.112 molH2, 0.112 molI2,...
An equilibrium mixture of H2, I2, and HI at 458 ∘C contains 0.112 molH2, 0.112 molI2, and 0.775 molHI in a 5.00-L vessel. Part A: What are the equilibrium partial pressure of HI when equilibrium is reestablished following the addition of 0.200 mol of HI? Express your answer to four significant figures and include the appropriate units. Part B:What are the equilibrium partial pressure of I2 when equilibrium is reestablished following the addition of 0.200 mol of HI? Express your...
At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this...
At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this temperature, 0.500 mol H2 and 0.500 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium?
Deriving concentrations from data The equilibrium constant, K, of a reaction at a particular temperature is...
Deriving concentrations from data The equilibrium constant, K, of a reaction at a particular temperature is detemined by the concentrations or pressures of the reactants and products at equilibrium. 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...
At a particular temperature, K = 7.40 × 102 for the reaction H2 (g) + 12 (g) 늑 2H1(g) In an experiment, 3.30 moles of H2, 3.30 moles of I2, and 3.30 moles of HI are introduced into a 1.00-L container Calculate the concentrations of all species when equilibrium is reached Concentration of H2 = Concentration of - Concentration ofHi-M
Equilibrium Concentrations -- A + B = 2C
At a particular temperature, K = 1.00×102
for the reaction:
H2(g) + F2(g)
2HF(g)
In an experiment, at this temperature, 1.00×10-1 mol
of H2 and 1.00×10-1 mol of F2 are
introduced into a 1.09-L flask and allowed to react. At
equilibrium, all species remain in the gas phase.
What is the equilibrium concentration (in mol/L) of
H2?
mol/L
1 pts
What is the equilibrium concentration (in mol/L) of HF?
mol/L
1 pts...
For the reaction below at a certain temperature, it is found
that the equilibrium concentrations in a 5.05-L rigid container are
[H2] = 0.0523 M, [F2] = 0.0121
M, and [HF] = 0.450 M.
H2(g) + F2(g) 2
HF(g)
If 0.203 mol of F2 is added to this equilibrium
mixture, calculate the concentrations of all gases once equilibrium
is reestablished.
Deriving concentrations from data The equilibrium constant, K, of a reaction at a particular temperature is detemined by the concentrations or pressures of the reactants and products at equilibrium. 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...
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