1. Arsenic can be extracted from its ores by first reacting the ores with oxygen (called roasting) to form solid As 06 which is then reduced using carbon according to the following equation: As 06(s) + 6 C(s) As4(g) + 6 CO (8)

Predict the direction of the shift of the equilibrium position in response to each of the following
changes in conditions.

A. addition of CO
B. removal of CO
C. removal of As4
D. addition of As4

they begin to vibrate harder causing the material that was solid to turn into a liquid i.e gallium or ice

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

20 drops hope this