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 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 separated by a comma. Express your answer using two significant figures.

Part C

Kp= 1.6×105

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

Answer #1

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= 1.6×10−4,Kp=
1.6×105,
Kp= 1.6×10−4 Pa, Pb= needed
Enter your answers numerically separated by a comma. Express
your answers using two significant figures.

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

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 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.

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

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.

For each strong acid solutions, determine [H3O+],[OH−],
and pH.
Please Answer all parts separately Will be very helpful
!!!
Part A
0.20 M HCl
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
[H3O+], [OH−] = ________________ M
Part B
Express your answer to two decimal places.
pH= _______________
Part C
1.6×10−2 M HNO3
Enter your answers numerically separated by a comma. Express
your answer using two significant figures.
[H3O+], [OH−] = ______________ M...

At 900 K the following reaction has Kp=0.345:
2SO2(g)+O2(g)⇌2SO3(g)
In an equilibrium mixture, the partial pressures of SO2 and O2
are 0.120 atm and 0.470 atm, respectively.
What is the equilibrium partial pressure of SO3 in the
mixture?
Express the pressure in atmospheres to three significant
digits.

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