If 0.200mol of nitrogen gas and 0.200mol of oxygen gas react, what is the limiting reactant?
N2(g)+O2(g)→2NO(g)
How many moles of NO are produced according to the equation?
Please show how to perform this equation with the answer please.
Here is how you do you it but you will need to go through and recalculate because I will do estimates only.
N2 + O2 ==> 2NO
Convert mols NH2 to mols NO using the coefficients in the balanced equation.
Thats 0.2 mol N2 x (2 mols NO/1 mol N2) = 0.2 x 2/1 = 0.4
Do the same with mols O2 to mols NO. That's 0.2 mols O2 x ( 2 mol NO/1 mol O2) = 0.2 x 2/1 = 0.4
There is no limiting reagent; both N2 and O2 react completely to form 0.4 mols NO.
How do I figure out the 2nd part? How many moles of NO are produced according to the equation?
I have watched several videos and I still don't understand this concept.
Re-read my response. Read it completely. Read it carefully. I told you how many mols NO were formed.
first answer is NO, and part B. is 2 mol
To determine the limiting reactant in a chemical reaction, you need to compare the stoichiometric ratios of the reactants to their actual amounts.
In this case, you are given that there are 0.200 moles of nitrogen gas (N2) and 0.200 moles of oxygen gas (O2).
Step 1: Convert the moles of N2 and O2 to moles of NO using the stoichiometric coefficients in the balanced equation:
N2(g) + O2(g) → 2NO(g)
According to the balanced equation, for every 1 mole of N2, 2 moles of NO are produced. Therefore, for 0.200 moles of N2, you can expect to produce 2 times 0.200 = 0.400 moles of NO.
Similarly, for every 1 mole of O2, 2 moles of NO are produced. So, for 0.200 moles of O2, you can anticipate producing 2 times 0.200 = 0.400 moles of NO.
Step 2: Compare the number of moles of NO produced from each reactant.
Since both the nitrogen gas and oxygen gas produce the same amount of moles of NO (0.400 moles in each case), neither reactant is limiting. In other words, both reactants are present in excess, and all of them will be used up to react completely.
To summarize, the limiting reactant is a reactant that is consumed fully, limiting the amount of product that can be produced. In this case, there is no limiting reactant as both N2 and O2 will be completely consumed. Therefore, you cannot determine the limiting reactant.
Finally, according to the balanced equation, 0.200 moles of nitrogen gas and 0.200 moles of oxygen gas will yield 0.400 moles of nitrogen monoxide (NO).