Can you explain when are we suppose to use an elements diatomic mass while doing

Question

Can you explain when are we suppose to use an elements diatomic mass while doing stoichiometry During the roasting of chalcocite, how many kg of oxygen are required to form 2.86 of copper I oxids 2.86 (v_2 U times 10^2g/10_y times |mol (v_2 U/|43.1v times 3md O2/2md times 32.00505/1mo_2 How may atoms are in 37 grams of oxygen 37 grams oxygen 1 mol/16 gram og times 6.022/|mol| oxygen Why in the first question we used 32 grams for the mars of oxygen and 16 grams for the second. Isn't oxygen diatomic on both question How would we know if a stiochimetry problem is asking for diatomic mass?

Explanation / Answer

2 Cu2S + 3O2 2 Cu2O + 2 SO2

286 gms of Cu2O is formed

3 moles of O2 gives 2 moles of Cu2O

1 mole of Cu2O = 143 gms

286 gms of Cu2O = 2 moles

It means 3 moles of O2 gives the required 2 moles of Cu2O

So, Mass of O2 = 96 gms = 0.096 Kg

1 mole of Oxygen = 32 gms

Oxygen is considered as a molecule [ O2]

1 mole = 32 gms = 6*10^23 atoms

37 gms contain = 6*10^23 *37/32 = 6.9375*10^23 atoms

In every chemical reaction we take oxygen as O2 ...

O is just the symbol of oxygen ; O2 is the molecule which is considered in reaction

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