2NO(g) + O2 (g) --> 2NO2
How many grams of NO are required to react fully with 5.00 mol of O2?
I do not understand any of this please help
To find the number of grams of NO required to react fully with 5.00 mol of O2, we need to use the balanced chemical equation and the concept of stoichiometry.
First, let's examine the balanced chemical equation:
2NO(g) + O2(g) -> 2NO2(g)
The coefficient in front of NO tells us that the stoichiometric ratio between NO and NO2 is 2:2 or 1:1. Therefore, for every 2 moles of NO, 2 moles of NO2 are formed.
Now, we need to determine the molar ratio between NO and O2. From the balanced equation, the molar ratio between NO and O2 is 2:1. This means that for every 2 moles of NO, we need 1 mole of O2 to react fully.
Given that there are 5.00 mol of O2, we can use the molar ratio to determine the required amount of NO.
Since the molar ratio is 2:1, we can set up the following proportion:
2 mol NO / 1 mol O2 = x mol NO / 5.00 mol O2
Using cross-multiplication, we find:
2 mol NO = 5.00 mol O2 * (2 mol NO / 1 mol O2)
2 mol NO = 10.00 mol NO
Therefore, 10.00 mol of NO are required to react fully with 5.00 mol of O2.
To convert this to grams, we need to use the molar mass of NO, which is approximately 30.01 g/mol.
To calculate the mass of NO required, we can use the following equation:
Mass of NO = moles of NO * molar mass of NO
Mass of NO = 10.00 mol * 30.01 g/mol
By multiplying these values together, we find that approximately 300.1 grams of NO are required to react fully with 5.00 mol of O2.
To determine the number of grams of NO required to react fully with 5.00 mol of O2, we can use the balanced equation and the molar ratio between NO and O2.
The balanced equation is:
2NO(g) + O2(g) --> 2NO2(g)
From the equation, we can see that 2 moles of NO react with 1 mole of O2. This means that the molar ratio between NO and O2 is 2:1.
So, in order to calculate the number of moles of NO required, we need to use this molar ratio.
Given:
Moles of O2 = 5.00 mol
Using the molar ratio, we can calculate the moles of NO required as follows:
Moles of NO = (Moles of O2) x (Molar ratio of NO : O2)
= 5.00 mol x (2 mol NO / 1 mol O2)
= 10.00 mol NO
Now, we can convert the moles of NO into grams using the molar mass of NO. The molar mass of NO is calculated as follows:
Molar mass of NO = (Molar mass of N) + (Molar mass of O)
= (14.01 g/mol) + (16.00 g/mol)
= 30.01 g/mol
Finally, we can calculate the grams of NO required:
Grams of NO = (Moles of NO) x (Molar mass of NO)
= 10.00 mol x (30.01 g/mol)
= 300.10 g
Therefore, to react fully with 5.00 mol of O2, you would need 300.10 grams of NO.
the reaction equation is written in MOLES
2 moles NO plus 1 mole O2 yields
... 2 moles NO2
so 5 moles of O2 uses 10 moles of NO
find the molar (formula) weight of NO, and multiply by 10