Given the following chemical equation, determine how many grams of N2 are produced by 8.58 g of H2O2 and 5.62 g of N2H4.
2H2O2(l)+N2H4(l)=4H2O(g)+N2(g)
This is a limiting reagent (LR) problem; you know that because amounts are given for BOTH reactants.
mols H2O2 = grams/molar mass = ?
mols N2H4 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols H2O2 to mols N2.
Do the same to convert mols N2H4 to mols N2.
It is likely that the numbers will not agree which means one of them is not right; the correct value in LR problems is ALWAYS the smaller value and the reagent responsible for that smaller value is the LR.
Now use the smaller value and convert that to grams. g = mols N2 x molar mass N2
To determine how many grams of N2 are produced, we'll need to use stoichiometry. Stoichiometry is a branch of chemistry that deals with the relative quantities of reactants and products in chemical reactions.
Step 1: Convert the given masses of H2O2 and N2H4 to moles:
To do this, we need to use the molar mass of each substance. The molar mass of H2O2 is 34.02 g/mol, and the molar mass of N2H4 is 32.05 g/mol.
For H2O2:
8.58 g H2O2 * (1 mol H2O2 / 34.02 g H2O2) = 0.2526 mol H2O2
For N2H4:
5.62 g N2H4 * (1 mol N2H4 / 32.05 g N2H4) = 0.1753 mol N2H4
Step 2: Determine the mole ratio of N2H4 to N2:
From the balanced equation, we can see that 1 mole of N2H4 reacts to produce 1 mole of N2. Therefore, the mole ratio of N2H4 to N2 is 1:1.
Step 3: Calculate the moles of N2 produced:
Since the mole ratio is 1:1, the moles of N2 produced will be equal to the moles of N2H4.
Moles of N2 produced = 0.1753 mol N2
Step 4: Convert the moles of N2 to grams:
To convert moles to grams, we need to use the molar mass of N2, which is 28.01 g/mol.
Grams of N2 = 0.1753 mol N2 * (28.01 g N2 / 1 mol N2) = 4.89 g N2
Therefore, approximately 4.89 grams of N2 are produced.