When 0.149 mol of carbon is burned in a closed vessel with
8.73 g
of oxygen, how many grams of carbon dioxide can form?
The reaction is:
C (s) + O2 (g) = CO2 (g)
Moles of C = 0.149 mole
Moles of O2 = Mass/ Molar mass = 8.73 g / (32 g / mole) = 0.273 mole
The reaction between C and O2 occurs at 1:1 mole ratio. So, here as the moles of C is less than the moles of O2, C is the limiting reagent.
Mole ratio of C : CO2 = 1:1
Moles of CO2 formed = Moles of C reacted = 0.149 mol
Mass of CO2 formed = 0.149 mole * Molar mass = 0.149 mole * 44 g/ mole = 6.56 g
When 0.149 mol of carbon is burned in a closed vessel with 8.73 g of oxygen,...
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