Oxides of virtually every element are known. bromine, for example, forms several oxides when treated with ozone. suppose you allow 1.250 g of bromine, br2, to react with ozone, o3, and obtain 1.876 g of brxoy. what is the empirical formula of the product?

Question

Rosa Weeks

Chemistry

27 October, 15:54

Oxides of virtually every element are known. bromine, for example, forms several oxides when treated with ozone. suppose you allow 1.250 g of bromine, br2, to react with ozone, o3, and obtain 1.876 g of brxoy. what is the empirical formula of the product?

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Miah Ayers · Answer 1

Answer is: empirical formula of the product is Br₂O₅.

Chemical reaction: x/2Br₂ + y/3O₃ → BrₓOy.

m (Br₂) = 1,250 g.

m (BrₓOy) = 1,876 g.

n (Br₂) = m (Br₂) : M (Br₂).

n (Br₂) = 1,25 g : 159,81 g/mol.

n (Br₂) = 0,0078 mol.

n (Br) = 2 · 0,0078 mol = 0,0156 mol.

m (O₃) = 1,876 g - 1,25 g = 0,626 g.

n (O₃) = 0,626 g : 48 g/mol = 0,013 mol.

n (O) = 0,039 · 3 = 0,039 mol

n (Br) : n (O) = 0,0156 mol : 0,039 mol.

n (Br) : n (O) = 1 : 2,5.