When 0.100 mol of carbon is burned in a closed vessel with 8.00g of oxygen, how many grams of carbon dioxide can form? Which reactant is in excess, and how many grams of it remain after the reaction?
please show all work and step by step solution
Balanced chmical reaction is
C + O2 CO2
molar mass of O2 = 32 gm/mole then 8 gm of O2 = 8/32 = 0.25 mole
According to reaction 1 mole of carbon react with 1 mole of threfore to react with 0.100 mole of carbon required oxygen = 0.100 mole but oxygen given 0.25 mole therefore oxygen is excess reactant
oxygen is excess reactant
required oxygen for reaction = 0.100 mole given =0.25 mole excess oxygen = 0.25 - 0.10 = 0.15 mole
molar mass of O2 = 32 gm/mole then 0.15 mole of O2 = 0.15 X 32 = 4.8 gm
4.8 gm of oxygen remain after reaction
According to reaction 1 mole of carbon produce 1 molel of carbon dioxide therefore 0.100 mole of carbon will produce 0.100 mole of carbon dioxide
molar mass of CO2 = 44.01 gm/mole then 0.100 mole of CO2 = 0.100 X 44.01 = 4.401 gm
4.401 gm of carbon dioxide form
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