Question

A mixture of 0.143 moles of C is reacted with 0.117 moles of O2 in a sealed, 10.0 L vessel at 500.0 K, producing a mixture of CO and CO2. The limiting reagent of the below reaction is carbon. 3C(s)+2O2​(g) CO2​(g)+2CO(g) For 0.143 moles of carbon, determine the amounts of products (both the CO and CO2) formed in this reaction. Also determine the amount of O2 remaining and the mole fraction for CO.

Answer 1

according to given reaction
number of mole of CO2 formed = (1/3)*(number of mole of C reacted)
= (1/3)*0.143
= 0.0477 mole

number of mole of CO formed = (2/3)*(number of mole of C reacted)
= (2/3)*0.143
= 0.0954 mole

number of O2 reacted = (2/3)*(number of mole of C reacted)
= (2/3)*0.143
= 0.0954 mole

number of mole of O2 remains = 0.177-0.0954
= 0.0816 mole

mole fraction of CO = moles of CO / total number of moles
= 0.0954 / (0.0477+0.0954+0.0816)
= 0.424