When 1.500 g of a metal oxide is heated, the compound decomposes in the reaction

Question

When 1.500 g of a metal oxide is heated, the compound decomposes in the reaction shown below.

2 M2O(s) ? 4 M(s) + O2(g)

If 0.1035 g O2 is produced, what is the identity of the metal?

Explanation / Answer

0.1035 g of O2 is produced =>(0.1035/16) moles of O2 is produced =>0.00646875 moles of O2 is produced This should be produced from 2*0.00646875 moles of metal oxide That is 0.0129375 Moles But given this many moles is equal to 1.5grams =>1 moles equals (1/0.0129375)*1.5 = 115.942 grams Let molecular weight of M be X Then (2X)+16 = 115.942 =>X = 49.97 grams So M is Vanadium

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