How much heat (in kilojoules) is evolved or absorbed in the reaction of 2.90g of Fe2O3 with enough carbon monoxide to produce iron metal? Fe2O3 + 3CO ---> 2Fe + 3CO2 dH=-24.8kJ How do you find q (of the 2Fe in kJ).
Given: *Fe2O3(s)+3CO(s)-->2Fe(s)+3CO2(g)(delta h is -23kJ) *3Fe2O3(s)+CO(g)-->2Fe3O4(s)+CO2(g)(delta h is -39kJ) *Fe3O4(s)+CO(g)-->3FeO(s)+CO2 (delta h is 18kJ) Desired:FeO(s)+CO(g)-->Fe(s)+CO2(g) find delta h for the
Please explain the answer. 1. Which statement about this reaction is correct? 2Fe(s)+3CO2(g)--->Fe2O3(s)+3CO(g) delta H = 26.6 kJ A. 26.6 kJ of energy are released for every mole of Fe reacted B. 26.6 kJ of energy are absorbed
Fe2O3+ 3CO=2Fe+3Co2, suppose that 1.64kg of Fe are obtained from a 2.62kg sample of Fe2O3 (ore). assuming that the reaction goes to completion, what is the percent purity of the Fe2O3 in the original sample.
Can you balance this equation please? Fe2O3 + CO yeilds Fe + CO2 Fe2O3 + CO ==> Fe + CO2 Rule: balance by changing coefficients. You may not change subscripts. Look at the Fe atoms. There are 2 Fe atoms on the left and only 1