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For the dissociation reaction: A2(g) ⇌ A2(g) is the equilibrium constant K=0.347 at the temperature T=300K,...
For the dissociation reaction: A2(g) ⇌ A2(g) is the equilibrium constant K=0.347 at the temperature T=300K, when the status of the standard is adopted (in other words partial pressure 1 bar for gases).
A) Calculate the ΔGr for the reaction at T=300K
B) calculate at which total pressure the molar fraction is 0.280 at 300K for the mixture.
Solutions
Amanda K answered 6 months agoRelated Solutions
The equilibrium constant, K , of a reaction at a particular temperature is determined by the...
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 in the...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, K, for the following reaction is 10.5
at 350 K.
2CH2Cl2(g) CH4(g) + CCl4(g) An equilibrium mixture of the three
gases in a 1.00 L flask at 350 K contains 5.47×10-2 M CH2Cl2, 0.177
M CH4 and 0.177 M CCl4. What will be the concentrations of the
three gases once equilibrium has been reestablished, if 3.44×10-2
mol of CH2Cl2(g) is added to the flask?
[CH2Cl2] =_____ M
[CH4] = ________M
[CCl4] =________ M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) =CH4(g) +...
The equilibrium constant, K, for the following reaction is
10.5 at 350 K.
2CH2Cl2(g)
=CH4(g) +
CCl4(g)
An equilibrium mixture of the three gases in a 1.00 L flask at
350 K contains
5.12×10-2 M
CH2Cl2,
0.166 M CH4 and
0.166 M CCl4. What
will be the concentrations of the three gases once equilibrium has
been reestablished, if 0.121 mol of
CH4(g) is added to the flask?
[CH2Cl2]
=
_________M
[CH4]
=
_________ M
[CCl4]
=
_________ M
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is...
At a particular temperature the equilibrium constant for the
reaction:
H2(g) + F2(g) ⇔ 2HF(g)
is K = 64.0. A reaction mixture in a 10.00-L flask contains 0.23
moles each of hydrogen and fluorine gases plus 0.50 moles of HF.
What will be the concentration of H2 when this mixture
reaches equilibrium?
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is...
At a particular temperature the equilibrium constant for the
reaction: H2(g) + F2(g) ⇔ 2HF(g) is K = 25.0. A reaction mixture in
a 10.00-L flask contains 0.33 moles each of hydrogen and fluorine
gases plus 0.30 moles of HF. What will be the concentration of H2
when this mixture reaches equilibrium?
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is...
At a particular temperature the equilibrium constant for the
reaction: H2(g) + F2(g) ⇔ 2HF(g) is K = 81.0. A reaction mixture in
a 10.00-L flask contains 0.25 moles each of hydrogen and fluorine
gases plus 0.37 moles of HF. What will be the concentration of H2
when this mixture reaches equilibrium?
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)...
At a certain temperature, this reaction establishes an
equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g)
<===> 4C(g) K(c) = 2.93 x 10^(27) If, at this temperature,
2.40 mol of A and 3.70 mol of B are placed in a 1.00-L container,
what are the concentrations of A, B, and C at equilibrium? [A] = ?
M [B] = ? M [C] = ? M
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)...
At a certain temperature, this reaction establishes an
equilibrium with the given equilibrium constant,
Kc.
3A(g) + 2B(g) <------> 4C(g)
Kc= 3.13x 10^31
If, at this temperature, 1.90 mol of A and 4.00 mol of B are placed
in a 1.00-L container, what are the concentrations of A, B, and C
at equilibrium?
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.
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...
At a certain temperature, the equilibrium constant, Kc, for this reaction is 2.60 SO2(g) + NO2(g)...
At a certain temperature, the equilibrium constant, Kc, for this
reaction is 2.60
SO2(g) + NO2(g) <--> SO3(g) + NO(g)
At this temperature, calculate the number of moles of NO2(g)
that must be added to 3.12 mol of SO2(g) in order to form 1.30 mol
of SO3(g) equilibrium
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