Fan and medal!!!! Carbon disulfide burns with oxygen to form carbon dioxide and sulfur dioxide in the following manner: CS2 + 3O2 CO2 + 2SO2 If 114 grams of CS2 are burned in an excess of O2 (an amount sufficient to completely burn all 114 g of CS2), how many moles of SO2 are formed? (Remember to follow significant figure rules).

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Fan and medal!!!! Carbon disulfide burns with oxygen to form carbon dioxide and sulfur dioxide in the following manner: CS2 + 3O2 CO2 + 2SO2 If 114 grams of CS2 are burned in an excess of O2 (an amount sufficient to completely burn all 114 g of CS2), how many moles of SO2 are formed? (Remember to follow significant figure rules).

Chemistry
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moles CS2 = 114 g/76.143 g/mol= 1.50 the ratio between CS2 and SO2 is 1 : 2 moles SO2 formed = 1.50 x 2 = 3.00

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