If 146.5g of chromium chlorate decomposes, what mass of oxygen can be produced?

The Equation for this reaction is as follow,

                                2 Cr(ClO₃)₃    →    2 CrCl₃  +  9 O₂
According to eq,

       604.68 g (2mole) of Cr(ClO₃)₃ produces  =  288 g (9 moles) of O₂
So,
                  146.5 g of Cr(ClO₃)₃ will produce  =  X g of O₂

Solving for X,
                              X  = (146.5 g × 288 g) ÷ 604.68 g

                              X  =  69.77 g of O₂

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