Question

Consider the following reaction:

A(g)⇌2B(g)

Find the equilibrium partial pressures of A and B for each of the
following different values of *K*p. Assume that the initial
partial pressure of B in each case is 1.0 atm and that the initial
partial pressure of A is 0.0 atm. Make any appropriate simplifying
assumptions.

*K*p= 1.6×10^{−4,}*K*p=
1.6×10^{5,}

*K*p= 1.6×10^{−4 Pa, Pb= needed}

Enter your answers numerically separated by a comma. Express your answers using two significant figures.

Answer #1

**a)**

**A ========== 2B**

**Initial 0 1**

**Final x (1-2x)**

** **

**Since the value is very small, hence the numerator will
be very small, hence the value of x will be close to 0.5 in this
case**

**The exact value of x in this case will be x=0.4955
(answer in two significant figures will either 0.49 or
0.50)**

**b)**

**A ========== 2B**

**Initial 0 1**

**Final x (1-2x)**

** **

**Since the value is very high, hence the denominator will
be very small, hence the value of x will be close to 0 in this
case**

**The exact value of x in this case will be x=6.2 *
10^(-6)**

Consider the following reaction: A(g)⇌2B(g) Find the equilibrium
partial pressures of A and B for each of the following different
values of Kp. Assume that the initial partial pressure of B in each
case is 1.0 atm and that the initial partial pressure of A is 0.0
atm. Make any appropriate simplifying assumptions.
Part A
Kp= 1.6
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
Part B
Kp= 2.0×10−4
Enter your answers numerically...

Consider the following reaction: A(g)⇌2B(g) Find the equilibrium
partial pressures of A and B for each of the following different
values of Kp. Assume that the initial partial pressure of B in each
case is 1.0 atm and that the initial partial pressure of A is 0.0
atm. Make any appropriate simplifying assumptions.
A) Kp= 2.0×10−4
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
B) Kp= 1.8×105
Enter your answers numerically separated by...

Consider the following reaction: A(g)⇌2B(g) Find the equilibrium
partial pressures of A and B for each of the following different
values of Kp. Assume that the initial partial pressure of B in each
case is 1.0 atm and that the initial partial pressure of A is 0.0
atm. Make any appropriate simplifying assumptions. Kp=1.8 Find Pa
and Pb.

Consider the reaction.
A(g)⇌2B(g)
Find the equilibrium partial pressures of A and Bfor each of the
different values of Kp. Assume that the initial partial
pressure of B in each case is 1.0 atm and that the initial partial
pressure of A is 0.0 atm. Make any appropriate simplifying
assumptions.
Part A
Kp= 2.4
Part B
Kp= 1.9×10−4
Part C
Kp= 1.8×105

A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for
each of the following different values of Kp. Assume that the
initial partial pressure of B in each case is 1.0 atm and that the
initial partial pressure of A is 0.0 atm. Make any appropriate
simplifying assumptions.
a)Kp= 2.0×105

Consider the following reaction:
A(g)⇌2B(g)
Find the equilibrium partial pressures of A and Bfor each of the
following different values of Kp. Assume that the initial
partial pressure of B in each case is 1.0 atm and that the initial
partial pressure of A is 0.0 atm. Make any appropriate simplifying
assumptions.
A) Kp= 1.6x10^-4
B) Kp=2.0X10^5

Consider the following reaction: A(g)⇌2B(g) Find the equilibrium
partial pressures of A and B for Kp=2.0 . Assume that the initial
partial pressure of B in each case is 1.0 atm and that the initial
partial pressure of A is 0.0 atm. Make any appropriate simplifying
assumptions.

At 1000 K, Kp = 19.9 for the reaction
Fe2O3(s)+3CO(g)?2Fe(s)+3CO2(g)
What are the equilibrium partial pressures of CO and CO2 if CO
is the only gas present initially, at a partial pressure of
0.904atm ?
Enter your answers numerically separated by a comma.

At 25 °C, the equilibrium partial pressures for the following
reaction were found to be PA = 5.11 atm, PB = 5.75 atm, PC = 4.98
atm, and PD = 4.91 atm. 2A(g)+2B(g)=C(g)+2D(g) What is the standard
change in Gibbs free energy of this reaction at 25 °C?

Consider the following reaction: A(g)⇌B(g)+C(g) Find the
equilibrium concentrations of A, B, and Cfor each of the following
different values of Kc. Assume that the initial concentration of A
in each case is 1.0 M and that the reaction mixture initially
contains no products. Make any appropriate simplifying
assumptions.
Kc= 1.2
Kc= 1.8x10−2
Kc= 2.0×10−5
Express your answer using two sig figs. Enter your answers
numerically seperated by commas.

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