Question

A reaction container holds 6.2g of P 4  and 8.0g of O 2 .The following reaction
occurs: P 4  + O 2   P 4 O 6 . If enough oxygen is available then the P 4 O 6  reacts
further: P 4 O 6  + O 2   P 4 O 10 . [ P=31,O =16]
a. What is the limiting reagent for the formation of P 4 O 10 ? 
b. What mass of P 4 O 10  is produced?  
c. What mass of excess reactant is left in the reaction container?

Answer 1

Answer:

The following quantities are placed in a container: 1.5 × 1024 molecules of diatomic hydrogen, 1.0 mol of sulfur, and 88.0 g of diatomic oxygen.

What is the total mass in grams for the collection of all three elements?

What is the total number of moles of atoms for the three elements?

If the mixture of the three elements formed a compound with molecules that contain two hydrogen atoms, one sulfur atom, and four oxygen atoms, which substance is consumed first?

How many atoms or molecules of each remaining element would remain unreacted in the change described above ?