Question

Time Remaining:03:23 1. Consider the balanced equation for the following reaction: 3Fe2O3(s) + CO(g) + CO2(g) + 2Fe3O4(s) How much excess reactant remains in the reaction if 46.8 grams of Fe2O3 reacts with 22.4 grams of CO? 0.195 moles 0.702 moles 0.800 moles 0.267 moles 0.507 moles Use the slider to rate your confidence on this question 100 Not at all confident Very confident

Answer 1

Number of moles of Fe2O3 = 46.8 g / 159.69 g/mol = 0.293 mole

Number of moles of CO = 22.4 g / 28.01 g/mol = 0.800 mole

From the balanced equation we can say that

3 mole of Fe2O3 requires 1 mole of CO so

0.293 mole of Fe2O3 will require

= 0.293 mole of Fe2O3 *(1 mole of CO / 3 mole of Fe2O3)

= 0.0977 mole of CO

But we have 0.800 mole of CO which is in excess so CO is an excess reactant

The number of moles of CO remains = 0.800 - 0.0977 = 0.702 mole

Therefore, the number of moles of CO remain after completion of reaction = 0.702