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a 6.0 g 6.0 g sample of carbon is burned to produce carbon dioxide. the yield from the reaction is only 60 % 60%. how much carbon dioxide was actually produced?

Sagot :

Carbon dioxide is created by burning a 6.0 g sample of carbon. The reaction only produces a 60% yield. Actual carbon dioxide production was 13.2g.

C + O2 = CO2

Moles of C in 6.0g = 6.0/12 =  0.5 moles

as 1 moles of C gives 1 mole of CO₂

Thus 0.5 moles of C will give 0.5 moles of CO₂

As, CO₂ produce is 60%

Thus, moles of CO₂ produced=(0.5x60)/100 = 0.3 moles of CO₂

Amount of CO2 produced=  Moles x Molecular mass

= 0.3 × 44

= 13.2g

Thus, 13.2g of CO₂ will be produced.

learn more about CO₂ here:

https://brainly.com/question/3049557

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