The gas arsine (ash3) decomposes as follows: 2ash3(g) < > 2as(s) + 3h2(g) in an experiment pure ash3(g) was placed in an empty, rigid, sealed flask at a pressure of 392.0 torr. after 48 h the pressure in the flask was observed to be constant at 488.0 torr. a. calculate the equilibrium pressure of h2(g). b. calculate kp for this reaction.

Answer :

(a) The equilibrium pressure of gas is, 288 torr

(b) The value for this reaction is, 0.786 atm

Solution :

The given equilibrium reaction is,

Initially pressure        392.0                           0

At equilibrium         (392.0-2x)                     3x

The final pressure in the flask after the reaction has completed is 488.0 torr. That means,

The partial pressure of at equilibrium = 3x = 3 × 96 = 288 torr

The partial pressure of at equilibrium = (392.0-2x) = [392.0-2(96)] = 200 torr

Now we have to calculate the for the reaction.

The expression of for the reaction will be:

Now put all the given values in this expression, we get:

Conversion used : (1 atm = 760 torr)

Therefore, the value for this reaction is, 0.786 atm

1. 1 mole of anything contains 6.022x10^23 pieces  

d  

2. a  

3. c, number  

5. 1.24x10^24atoms / 6.022x10^23atoms/mole = 2moles h2 atoms  

6. fe2br3 mass = 2moles x mass fe + 3 moles x mass br  

molar mass = grams / number of moles = g/mole  

to find moles = g / molar mass  

to find mass = g = molar mass / moles

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i