Zinc(II) sulfide reacts with oxygen according to the reaction:  2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g)2ZnS(s)+3O2(g)→2ZnO(s)+2SO2(g) A reaction mixture initially contains 3.8 molmol ZnSZnSand 6.3 molmol O2O2 Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?         Express your answer using one significant figure.

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