Use the balanced equation, N2 + O2 --> 2NO, to answer the following questions...
A) How many grams of NO are formed from 10.0g of N2?
I really don't know how to do this, so please show work so i know. There are more questions to this question but i want to see how it works.
N2 + O2 --> 2NO
mols N2 = grams/molar mass = 10/28 = approx 0.3 but you need a more accurate answer than that estimate.
Use the balanced equation to convert mols N2 to mols NO. That's 0.3 x (2 mols NO/1 mol N2) = approx 0.3 x 2/1 = approx 0.6 mol NO.
Then grams NO = mols NO x molar mass NO = ?
Thanks for the help! I around my answer to 4 sig figs, so my answer is 21.4 g of NO. thanks for the help again!
I meant 3 sig figs.
To solve this problem, you need to apply stoichiometry, which involves using the balanced equation to determine the relationship between the reactants and products.
Step 1: Determine the molar mass of N2 and NO
The molar mass of N2 is 28.02 g/mol (14.01 g/mol x 2).
The molar mass of NO is 30.01 g/mol (14.01 g/mol + 16.00 g/mol).
Step 2: Convert grams to moles
Use the molar mass of N2 to convert grams of N2 to moles.
10.0 g N2 x (1 mol N2 / 28.02 g N2) = 0.356 mol N2
Step 3: Apply stoichiometry
From the balanced equation, we can see that the ratio between N2 and NO is 1:2. This means that for every mole of N2, we get 2 moles of NO.
So, we can calculate the number of moles of NO produced by multiplying the moles of N2 by the stoichiometric ratio.
0.356 mol N2 x (2 mol NO / 1 mol N2) = 0.712 mol NO
Step 4: Convert moles to grams
Finally, we can convert the moles of NO to grams using its molar mass.
0.712 mol NO x (30.01 g NO / 1 mol NO) = 21.37 g NO
Therefore, from 10.0 g of N2, we can expect to produce 21.37 g of NO.