In a study of the following reaction at 1200 k it was observed that when the equilibrium partial pressure of water vapor is 15.0 torr, the total pressure at equilibrium is 36.3 torr. 3 fe(s) 4 h2o(g) equilibrium reaction arrow fe3o4(s) 4 h2(g) calculate the value of kp for this reaction at 1200 k. hint: apply dalton's law of partial pressures.

The value of for this reaction at 1200 K is 4.066.

Explanation:

Partial pressure of water vapor at equilibrium =

Partial pressure of hydrogen gas at equilibrium =

Total pressure of the system at equilibrium P = 36.3 Torr

Applying Dalton's law of partial pressure to determine the partial pressure of hydrogen gas at equilibrium:

The expression of is given by:

The value of for this reaction at 1200 K is 4.066.

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