6.0 moles of `Fe_(2)O_(3)` (s) reacts with 9.0 moles of carbon in a blast furnace according to the equation given below. `Fe_(2)O_(3)`(s)+ 3C(s)→2Fe(s)+3CO(g) What is the theoretical yield of Fe in moles?

Name the four man zones of blast furnace in the extraction of Fe from Fe_(2)O_(3) .

What is the value of Delta s^(@) for the reaction below? Fe_(2)O_(3)(s)+3CO(g)to2Fe(s)+3CO_(2)(g)

Fe_(2)O_(3) reacts with excess CO at a high temperature according to the equation below: Fe_(2)O_(3) + 3CO rightarrow 2Fe + 3CO_(2) If 6.5-0g of Fe_(2)O_(3) yields 3.85g of Fe, what is the percentage yield of the reaction ?

The number of moles of Fe_(2)O_(3) formed when 0.5 moles of O_(2) and 0.5 moles of Fe are allowed to react are

The number of moles of Fe_(2)O_(3) formed when 0.5 moles of O_(2) and 0.5 moles of Fe are allowed to react are

How many moles of iron can be made from Fe_(2)O_(3) by the use of 16 mol of carbon monoxide in the following reaction : Fe_(2)O_(3) + 3CO to 2Fe + 3CO_(2)

For the reaction Fe_2N(s)+(3)/(2)H_2(g)=2Fe(s)+NH_3(g)

One mole mixture of FeO and Fe_(3)O_(4) containing equal moles of each on reaction with excess O_(2) gives n moles of Fe_(2)O_(3).n is:

Write a balanced chemical equation : FeSO_(4)(s) overset("Heat")to Fe_(2)O_(3)(s) +SO_(2)(g) +SO_(3)(g)