Small amounts of oxygen gas can be produced for laboratory use by heating potass

Question

Small amounts of oxygen gas can be produced for laboratory use by heating potassium chlorate, which causes it to decompose by the following reaction: ___KClO3(s) ? ____KCl(s) + ___O2(g) (unbalanced) Balance the equation, and determine the mass of oxygen that will be formed if 10.0 g of potassium chlorate decomposes. Answer                              A. 38.3 g                 B. 57.4 g                 C. 3.92 g                 D. 115 g                 E. 7.83 g Small amounts of oxygen gas can be produced for laboratory use by heating potassium chlorate, which causes it to decompose by the following reaction: ___KClO3(s) ? ____KCl(s) + ___O2(g) (unbalanced) Balance the equation, and determine the mass of oxygen that will be formed if 10.0 g of potassium chlorate decomposes. ___KClO3(s) ? ____KCl(s) + ___O2(g) (unbalanced) Balance the equation, and determine the mass of oxygen that will be formed if 10.0 g of potassium chlorate decomposes. 38.3 g 57.4 g 3.92 g 115 g 7.83 g                 A. 38.3 g                 B. 57.4 g                 C. 3.92 g                 D. 115 g                 E. 7.83 g

Explanation / Answer

2KClO3(s) ------> 2KCl(s) + 3O2(g)

(2*122.55)                        (3*32)

M.wt of KClO3 =122.55

M.wt of O2 =32

245.1 g of KClO3 produes 96 g of oxygen

10 g of KClO3 produes = (96*10/245.1)

                                 = 3.9168 g

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