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Brut [27]
3 years ago
14

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
Chemistry
2 answers:
SVETLANKA909090 [29]3 years ago
6 0
Given:
<span>CS2 + 3O2 → CO2 + 2SO2
</span><span>114 grams of CS2 are burned in an excess of O2
</span>
moles CS2 = 114 g/76.143 g/mol → 114g * mol/76.143 g =  1.497 mol

<span>the ratio between CS2 and SO2 is 1 : 2 </span>

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

MA_775_DIABLO [31]3 years ago
5 0

Answer:

B

Explanation:

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<h2>2.49 g/cm³</h2>

Explanation:

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3 0
2 years ago
What is the ph of a 0.0055 m ha (weak acid) solution that is 8.2% ionized?
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3 0
3 years ago
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mestny [16]

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6 0
3 years ago
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8 0
2 years ago
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