of exhow many grams of no2 can be produced by the reaction of excess o2 with 19.8 of no
Here is an worked example. Just follow the steps. I would learn how to spell chemistry, how to write formulas no spells "no" (the opposite of yes) to me. Finally, I would learn to start sentences with a capital letter and end them with a period. You will get more answers that way.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Post your work if you get stuck.
To determine the number of grams of NO2 that can be produced by the reaction of excess O2 with 19.8 grams of NO, you need to use stoichiometry and the balanced chemical equation for the reaction. Here's how you can calculate it:
1. Begin by writing down the balanced chemical equation for the reaction.
2 NO + O2 -> 2 NO2
2. Use the molar mass of NO to convert the given mass of NO to moles. The molar mass of NO is 30 g/mol.
19.8 g NO x (1 mol NO / 30 g NO) = 0.66 mol NO
3. Apply stoichiometry to determine the moles of NO2 produced. From the balanced equation, you can see that 2 moles of NO react to produce 2 moles of NO2.
0.66 mol NO x (2 mol NO2 / 2 mol NO) = 0.66 mol NO2
4. Convert the moles of NO2 to grams by using the molar mass of NO2. The molar mass of NO2 is 46 g/mol.
0.66 mol NO2 x (46 g NO2 / 1 mol NO2) = 30.36 g NO2
Therefore, when excess O2 reacts with 19.8 grams of NO, you can produce 30.36 grams of NO2.