The molar mass of iron oxide (fe2o3) is 159.7 g/mol. what is the correct way to write the molar mass of iron oxide as a conversion factor?

or

Explanation: Given molar mass of Iron(III)oxide is 159.7 g/mol. It means the mass of 1 mol of Iron(III)oxide is 159.7 g.

How to write the molar mass as a conversion factor is all depends if we are calculating the moles or grams.

If the grams are given and we are asked to calculate the moles then the conversion factor is written as and if the moles are given and we are asked to calculate the grams then the conversion factor is written as .

c 159.7g Fe2 O3/ 1 mol Fe2 O 3

Explanation:

I just did it:)

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

because natural gas is colorless, odorless, and tasteless, distributors add mercaptan (a chemical that smells like sulfur) to give natural gas a distinct unpleasant odor (it smells like rotten eggs). they locate the types of rock that are likely to contain natural gas deposits.