Consider the reaction 4FeS2 + 11O2 → 2Fe2O3 + 8SO2. If 8 moles of FeS2 react with 15 moles of O2, what is the limiting reactant?

FeS_2

Fe_2O_3

O_2

SO_2

(The underscores with the number represents the number being subscripted)

The limiting reactant is .

Explanation:

Both nor are on the right-hand side of the equation; these two species are products, not reactants. The only two reactants are and .

Assume that is the limiting reactant, such that all of its formula units are consumed. That is: .

In the balanced equation, the ratio between the coefficient of and that of is:

.

Apply this ratio to find the number of moles of consumed, assuming that is the limiting reactant:

.

In other words, of would be required to consume all that of formula units. However, only of was available. Therefore, some formula units would not have been consumed; would be the reactant in excess, whereas would be the limiting reactant.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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