If 0.25 moles of O2 and 0.55 moles of NO are used, how much NO2 will
be produced? O2 + 2NO - 2NO2
2 answers
I really need help with this!!
O2 + 2NO - 2NO2
When amounts are given for both reactants you know it is a limiting reagent (LR) problem; i.e., one of the reactants will be used completely and there will be some of the other reactant left unreacted.
Try both. Since 1 mole O2 will require 2 moles NO, you know that 0.25 moles will require 0.50 moles NO. Do you have much NO? Yes, so O2 will be the LR and some NO will be unused. What if we asked that question and started with NO. Since 2 moles NO will require 1 mol O2, then 0.55 moles NO will require 0.55/2 or 0.275 moles O2. Do we have that much O2? NO, therefore, O2 will be the imiting reagent and NO will not be used completely. To continue, now that we know which is the LR, we know to work with O2 and not NO. We know 1 mole O2 will produce 2 mols NO2; therefore, 0.25 moles O2 will produce 0.50 moles NO2. If you want to know grams, then grams NO2 = moles NO2 x molar mass NO2 = ?
When amounts are given for both reactants you know it is a limiting reagent (LR) problem; i.e., one of the reactants will be used completely and there will be some of the other reactant left unreacted.
Try both. Since 1 mole O2 will require 2 moles NO, you know that 0.25 moles will require 0.50 moles NO. Do you have much NO? Yes, so O2 will be the LR and some NO will be unused. What if we asked that question and started with NO. Since 2 moles NO will require 1 mol O2, then 0.55 moles NO will require 0.55/2 or 0.275 moles O2. Do we have that much O2? NO, therefore, O2 will be the imiting reagent and NO will not be used completely. To continue, now that we know which is the LR, we know to work with O2 and not NO. We know 1 mole O2 will produce 2 mols NO2; therefore, 0.25 moles O2 will produce 0.50 moles NO2. If you want to know grams, then grams NO2 = moles NO2 x molar mass NO2 = ?
4 answers