Consider an open system that is in equilibrium with 10^-2 atm CO2
(g). You have no...
Consider an open system that is in equilibrium with 10^-2 atm CO2
(g). You have no other information about the system. Henry's Law
telss us that KhCI2=H2CO3/pCO2= 10^-1.5 M-atm^-1
pKa1 is 6.3 (for H2CO3* dissassociation) and pKa2 is 10.3 (for
HCO3- dissassociation). What is the [HCO3*], and [CO3^2-] if the pH
of the solution is 5, 7,9?
Solutions
Expert Solution
Here we used henry's law relation, ph relation and dissociation
. Now just calculate the substituted values.
A system at equilibrium contains I 2 (g) at a pressure of 0.19
atm and I(g) at a pressure of 0.22 atm . The system is then
compressed to half its volume. Part A Find the pressure of I 2 when
the system returns to equilibrium. Part B Find the pressure of I
when the system returns to equilibrium.
Consider the following equilibrium.
CS2(g) + 3 O2(g) equilibrium reaction arrow CO2(g) + 2 SO2(g)
If the reaction is started in a container with 5.59 atm CS2 and
13.3 atm O2, what is Kp if the partial pressure of CO2 is 3.76 atm
at equilibrium? (There is no change in temperature and the initial
partial pressures of the products are equal to 0.)
A water is in equilibrium with CO2 in the atmosphere (partial
pressure is 3.16 .10‾⁴atm) and with CaCO3(s). The pH is 8.1.
Ignoring Ca complexes, what is the
solubility (S) of Ca?
The system
CO2(g) + H2(g) H2O(g) + CO(g)
is at equilibrium at some
temperature. At equilibrium, a 4.00L vessel contains 1.00 mole CO2,
1.00 mole H2, 2.40 moles H2O, and 2.40 moles CO. How many moles of
CO2 must be added to this system to bring the equilibrium CO
concentration to 0.669 mol/L?
A. 0.498 moles
B.
0.993 moles
C.
0.429 moles
D.
0.069 moles
Consider the reaction: NO2 (g) + CO (g) --->
CO2 (g) + NO (g)
The equilibrium constant is at 701 K and 895 K are 2.57 and 567
L mol-1 s-1 so,
A. Find the reaction order
B. Energy of Activation
C. Use part b to find the reaction rate constant at 200
C
A system at equilibrium contains I2(g) at a pressure of
0.25 atm and I(g) at a pressure of 0.25 atm . The system
is then compressed to half its volume.
Part A
Find the pressure of I2 when the system returns to
equilibrium.
Express your answer to two significant figures and include the
appropriate units.
Part B
Find the pressure of I when the system returns to
equilibrium.
Express your answer to two significant figures and include the
appropriate units.
A system at equilibrium contains I2(g) at a pressure of
0.13 atm and I(g) at a pressure of 0.18 atm . The system
is then compressed to half its volume.
Part A
Find the pressure of I2 when the system returns to
equilibrium.
Part B
Find the pressure of I when the system returns to
equilibrium.
A system at equilibrium contains I2(g) at a pressure of
0.18 atm and I(g) at a pressure of 0.21 atm .
The system is then compressed to half its volume.
Part A
Find the pressure of I2 when the system returns to
equilibrium.
Part B
Find the pressure of I when the system returns to
equilibrium.
23.Consider the following equilibrium process at
686°C:
CO2(g) + H2(g) ⇌
CO(g) + H2O(g)
The equilibrium concentrations of the reacting species are
[CO] = 0.0580 M,
[H2] = 0.0430
M,
[CO2] = 0.0900 M,
and [H2O] = 0.0420
M.
(a) Calculate Kc for
the reaction at 686°C.
________
(b) If we add CO2 to increase
its concentration to 0.460 mol / L, what will the concentrations of
all the gases be when equilibrium is reestablished?
CO2:
M
H2:
M
CO:...
For the equilibrium
2IBr(g)?I2(g)+Br2(g)
Kp=8.5×10?3 at 150 ?C.
A) If 2.1×10?2 atm of IBr is placed in a 2.0-L
container, what is the partial pressure of IBr after equilibrium is
reached?
Express your answer to two significant figures and include the
appropriate units.
B) If 2.1×10?2 atm of IBr is placed in a 2.0-L
container, what is the partial pressure of I2 after equilibrium is
reached?
Express your answer to two significant figures and include the
appropriate units.
C) If...