If 0.25 moles of O2 and 0.55 moles of NO are used, how much NO2 will
be produced? O2 + 2NO - 2NO2
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 = ?
I really need help with this!!
To find out how much NO2 will be produced when 0.25 moles of O2 and 0.55 moles of NO are used, we need to determine the limiting reagent first. The limiting reagent is the reactant that is completely consumed and determines the maximum amount of product that can be formed.
To determine the limiting reagent, we compare the number of moles of each reactant to the stoichiometric ratio given in the balanced equation. The balanced equation tells us that 1 mole of O2 reacts with 2 moles of NO to produce 2 moles of NO2.
Let's calculate the moles of NO2 that can be formed from 0.25 moles of O2 and 0.55 moles of NO:
Moles of NO2 from O2 = 0.25 moles O2 × (2 moles NO2 / 1 mole O2) = 0.5 moles NO2
Moles of NO2 from NO = 0.55 moles NO × (2 moles NO2 / 2 moles NO) = 0.55 moles NO2
Now, we compare the moles of NO2 produced from each reactant. Since the number of moles of NO2 from O2 is 0.5 moles and the number of moles of NO2 from NO is 0.55 moles, the limiting reagent is O2.
Therefore, the maximum amount of NO2 that can be produced is 0.5 moles.
Note: The stoichiometry of the balanced equation tells us that for every 1 mole of O2, we can produce 2 moles of NO2. However, since O2 is the limiting reagent, we only have enough O2 to produce 0.5 moles of NO2.