In: Chemistry

# At a certain temperature, 0.860 mol of SO3 is placed in a 1.50-L container. At equilibrium,...

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.

## Solutions

##### Expert Solution

Answer – Given, moles of SO3 = 0.860 , volume = 1.50 L , at equilibrium moles of O2 = 0.100 moles

We know reaction –

2 SO3 ---> 2 SO2 + O2

First we need to calculate the molarity

[SO3] = 0.860 mole / 1.50 L = 0.573 M

[O2] = 0.10 mole / 1.5 L = 0.0667 M

Now we need to put ICE chart

2 SO3 ---> 2 SO2 + O2

I   0.573           0         0

C    -2x            +2x     +x

E 0.573-2x      +2x     0.0667

So, x = 0.0667 M

So, at equilibrium,

[SO3] = 0.573-2x

= 0.573 -2*0.0667

= 0.440 M

[SO2] = 2x

= 0.133 M

[O2] = x = 0.0667 M

So, Kc = [SO2]2[O2] / [SO3]2

= (0.133)2*90.0667) / (0.44)2

= 0.00612

## Related Solutions

##### At a certain temperature, 0.680 mol of SO3 is placed in a 3.50-L container. 2SO3 (g)...
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...
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)...
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...
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...
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...
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...
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...
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...
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...
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?