Nitrogen oxide reacts with oxygen gas to form nitrogen dioxide (NO2). In one experiment 0.866 mole of NO is mixed with 0.503 mole of O2. Calculate the number of moles of NO2 produced
This is a limiting reagent problem. I know that because an amount for BOTH reactants is given.
2NO + O2 ==> 2NO2
mols NO = 0.866
mols O2 = 0.503
Convert mols NO to mols NO2. Use the coefficients. That's 0.866 x (2 mols NO2/2 mols NO) = 0.866 x 2/2 = 0.866
Convert mols O2 to mols NO2. That's
0.503 x (2 mols NO2/1 mol O2) = 0.503 x 2/1 = 1.006
You know both answers (0.866 and 1.006) can't be right and one of them must be wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent. Therefore the NO is the limiting reagent and you will produce 0.866 mol NO2.
Well, this reaction seems to be quite explosive in terms of moles! Let's balance the equation first:
2 NO + O2 → 2 NO2
Now that we have the balanced equation, we can see that it takes two moles of NO to react with one mole of O2 to produce two moles of NO2.
Since we have 0.866 moles of NO, and each mole of NO will react to produce 1 mole of NO2, we can say that 0.866 moles of NO will produce 0.866 moles of NO2.
But hold on, we also have 0.503 moles of O2, and we know that O2 is the limiting reagent here since we don't have enough of it to react with all the NO. Since it takes one mole of O2 to react with two moles of NO, we can say that 0.503 moles of O2 will react with 0.2515 moles of NO to produce 0.503 moles of NO2.
Therefore, the total moles of NO2 produced in this reaction will be the sum of the moles produced from NO and O2:
0.866 moles + 0.503 moles = 1.369 moles
So, approximately 1.369 moles of NO2 will be produced in the reaction.
To determine the number of moles of NO2 produced, we need to use the balanced chemical equation for the reaction between nitrogen oxide (NO) and oxygen gas (O2) to form nitrogen dioxide (NO2).
The balanced chemical equation is:
2NO + O2 -> 2NO2
From the equation, we can see that 2 moles of NO react with 1 mole of O2 to produce 2 moles of NO2.
Given that we have 0.866 moles of NO and 0.503 moles of O2, we need to determine which reactant (NO or O2) is limiting.
To do this, we'll compare the moles of NO and O2. Divide the number of moles of each reactant by the respective stoichiometric coefficient in the balanced equation:
Moles of NO2 produced from NO: 0.866 moles of NO x (2 moles of NO2 / 2 moles of NO) = 0.866 moles of NO2
Moles of NO2 produced from O2: 0.503 moles of O2 x (2 moles of NO2 / 1 mole of O2) = 1.006 moles of NO2
Since 0.866 moles of NO produce a smaller amount of NO2 compared to 0.503 moles of O2, it means that NO is the limiting reactant.
Therefore, in this experiment, the number of moles of NO2 produced is 0.866 moles.
To calculate the number of moles of NO2 produced, we first need to determine the limiting reactant. The limiting reactant is the one that will be completely consumed, limiting the amount of product that can be formed.
To find the limiting reactant, we need to compare the number of moles of each reactant to their stoichiometric coefficients in the balanced chemical equation.
The balanced chemical equation for the reaction is:
2 NO + O2 → 2 NO2
From the equation, we can see that 2 moles of NO are required to react with 1 mole of O2 to produce 2 moles of NO2.
Now, let's compare the moles of each reactant we have:
NO: 0.866 moles
O2: 0.503 moles
Let's start by comparing the moles of NO and O2 based on their stoichiometric coefficients:
Moles of NO required = 2 * Moles of O2
Moles of NO required = 2 * 0.503 moles = 1.006 moles
Since we have 0.866 moles of NO, which is less than 1.006 moles required, NO is the limiting reactant.
Now that we know that NO is the limiting reactant, we can use the stoichiometry of the balanced equation to find the number of moles of NO2 produced.
According to the balanced equation, 2 moles of NO produce 2 moles of NO2. Therefore, the ratio of moles of NO2 to moles of NO is 1:1.
Since NO is the limiting reactant, the moles of NO2 produced will be equal to the moles of NO consumed.
Therefore, the number of moles of NO2 produced is 0.866 moles.
So, in this experiment, 0.866 moles of NO2 is produced.