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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).

Question

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).

anonymous · Answer

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