In part a, you found the amount of product (3.80 mol p2o5 ) formed from the given amount of phosphorus and excess oxygen. in part b, you found the amount of product (3.40 mol p2o5 ) formed from the given amount of oxygen and excess phosphorus. now, determine how many moles of p2o5 are produced from the given amounts of phosphorus and oxygen. express your answer to three significant figures and include the appropriate units. view available hint(s)

The balanced chemical equation between phosphorus and oxygen can be given as,

3.80 mol is formed from P (limiting reactant):

Moles of P =

3.40 mol is produced when Oxygen is limiting:

Moles of =

So we have 7.6 mol P and 8.5 mol O2.

Calculating the moles of P2O5 formed from the given moles of P and O2:

Moles of phosphorus pentoxide from P =

So the moles of produced from P are

=

Moles of phosphorus pentoxide formed from O2 =

O2 produced the least amount of the product so oxygen would be the limiting reactant.

Moles of produced will be 3.40 mol

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

24

no statements shown

the atomic number of carbon is six, which means that a carbon atom has six protons. carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. which of these statements are true about carbon and its isotopes? select all that appl