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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 burn completely all 114 g of CS2), how many moles of SO2 are formed

2.50
2.99
2.00
1.00
50.00

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BlueSky06
Given:
CS2 + 3O2 → CO2 + 2SO2
114 grams of CS2 are burned in an excess of O2

moles CS2 = 114 g/76.143 g/mol → 114g * mol/76.143 g =  1.497 mol

the ratio between CS2 and SO2 is 1 : 2 

moles SO2 formed = 1.497 x 2 = 2.994 moles   → 2nd option

Answer:

B

Explanation:

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