In: Chemistry

At a certain temperature, 0.860 mol of SO3 is placed in a 1.50-L container. At equilibrium, 0.100 mol of O2 is present. Calculate Kc.

**Answer** – Given, moles of SO_{3} = 0.860
, volume = 1.50 L , at equilibrium moles of O_{2} = 0.100
moles

We know reaction –

2 SO_{3} ---> 2 SO_{2} + O_{2}

First we need to calculate the molarity

[SO_{3}] = 0.860 mole / 1.50 L = 0.573 M

[O_{2}] = 0.10 mole / 1.5 L = 0.0667 M

Now we need to put ICE chart

2 SO_{3} ---> 2 SO_{2} +
O_{2}

I 0.573 0 0

C -2x +2x +x

E 0.573-2x +2x 0.0667

So, x = 0.0667 M

So, at equilibrium,

[SO_{3}] = 0.573-2x

= 0.573 -2*0.0667

= 0.440 M

[SO_{2}] = 2x

= 0.133 M

[O_{2}] = x = 0.0667 M

So, **Kc** =
[SO_{2}]^{2}[O_{2}] /
[SO_{3}]^{2}

=
(0.133)^{2}*90.0667) / (0.44)^{2}

=
**0.00612**

At a certain temperature, 0.680 mol of SO3 is placed in a 3.50-L
container. 2SO3 (g) <---> 2SO2(g) +O2(g) At equilibrium,
0.190 mol of O2 is present. Calculate Kc.

14) At a certain temperature, 0.920 mol of SO3 is placed in a
4.50-L container. 2So3 (g) <--> 2SO2 (g) + O2 (g) At
equilibrium, 0.200 mol of O2 is present. Calculate Kc.

At a certain temperature, 0.920 mol of SO3 is placed in a 4.00-L
container. 2SO3(g) <===>2SO2(g) + O2(g) At equilibrium, 0.130
mol of O2 is present. Calculate Kc.

At a certain temperature, 0.900 mol SO3 is placed in a 5.00 L
container.
2SO3(g)−⇀↽−2SO2(g)+O2(g)
At equilibrium, 0.110 mol O2 is present. Calculate Kc.

A certain quantity of HI was placed in a 1.00 L container, when
equilibrium is reached [I2]=1.8 and kc= 6., what was the original
number of moles of Hi placed in the reaction flask?
***please show all work... i want to understand how to do it

A 0.831 gram sample of SO3 is placed in a 1.00 L
rigid container and heated to 1100 K. The SO3 decomposes
to SO2 and O2 :
2SO3(g) ↔ 2SO2(g) + O2(g)
At equilibrium, the total pressure in the container is 1.300
atm. Calculate the value of Kp at 1100 K
Extra Credit: Consider two
containers A and B where A is a rigid container and B is a
container with a massless, frictionless piston that maintains
constant pressure....

1.00 mol of A and 1.00 mol of B are placed in a 4.00-L
container. After equilibrium is established, 0.400 mol of D is
present in the container. Calculate the equilibrium constant for
the reaction: A(g) + 3 B(g) <---> C(g) + 2 D(g)

At a certain temperature, 0.332 mol of CH4 and 0.953 mol of H2S
is placed in a 2.00 L container.
At equilibrium, 14.3 g of CS2 is present. Calculate Kc.

At a certain temperature, 0.4011 mol of N2 and 1.581 mol of H2
are placed in a 1.50L container. N2(g) + 3H2(g) −⇀↽− 2NH3(g) At
equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium
constant, Kc.

2.00 moles of CO2 and 1.50 moles of H2 are placed into a rigid
5.00-L container and they react according to the equation ? ?
CO2(g) + H2(g) ? CO(g) + H2O(g) ? ? K = 2.50 What will be the
concentration of carbon monoxide when equilibrium is reached?

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