How many moles of oxygen are needed to react with 170 g of hydrazine?
Well, let's calculate it! To find the number of moles of oxygen needed, we need to know the balanced chemical equation for the reaction between hydrazine (N2H4) and oxygen (O2). So, let me grab my fancy chemistry hat... *puts on a clown wig* Okay, I'm ready!
The balanced equation for the reaction is:
N2H4 + O2 -> N2 + 2H2O
From the equation, we can see that 1 molecule of hydrazine (N2H4) reacts with 1 molecule of oxygen (O2).
Now, the molar mass of hydrazine (N2H4) is approximately 32 g/mol, so 170 g would be equal to 170/32 = 5.31 moles of hydrazine.
Since the ratio of hydrazine to oxygen is 1:1, we would need 5.31 moles of oxygen to react with 170 g of hydrazine. But remember, that's only if the oxygen shows up for the reaction and doesn't bail out early!
I hope I've shed some light on this with my clown chemistry act! *honks nose*
To determine the number of moles of oxygen needed to react with 170 g of hydrazine, we need to follow these steps:
Step 1: Find the molar mass of hydrazine (N2H4)
The molar mass of N2H4 can be calculated by adding up the atomic masses of each element:
Molar mass of N2H4 = (2 x atomic mass of nitrogen) + (4 x atomic mass of hydrogen)
The atomic mass of nitrogen (N) is approximately 14 g/mol, and the atomic mass of hydrogen (H) is approximately 1 g/mol.
Molar mass of N2H4 = (2 x 14 g/mol) + (4 x 1 g/mol) = 32 g/mol
Step 2: Convert mass of hydrazine to moles
We can use the formula:
Number of moles = Mass / Molar mass
Number of moles of hydrazine = 170 g / 32 g/mol ≈ 5.31 mol
Step 3: Determine the stoichiometry of the reaction
The balanced equation for the reaction between hydrazine (N2H4) and oxygen (O2) is:
N2H4 + O2 → N2 + 2H2O
From the balanced equation, we can see that the stoichiometric ratio between hydrazine and oxygen is 1:1. Therefore, for every mole of hydrazine, we need 1 mole of oxygen.
Step 4: Calculate the moles of oxygen needed
Since the stoichiometric ratio is 1:1, the number of moles of oxygen needed is the same as the number of moles of hydrazine, which is 5.31 moles.
Therefore, 5.31 moles of oxygen are needed to react with 170 g of hydrazine.
To determine the number of moles of oxygen needed to react with 170 g of hydrazine, we need to first determine the balanced chemical equation for the reaction between hydrazine (N2H4) and oxygen (O2).
The balanced chemical equation for the reaction is:
N2H4 + O2 → N2 + 2 H2O
From the balanced equation, we can see that for every 1 mole of hydrazine (N2H4), we need 1 mole of oxygen (O2) to react. This means the mole ratio between N2H4 and O2 is 1:1.
Now, we need to calculate the number of moles of hydrazine in 170 g. To do this, we need to know the molar mass of hydrazine (N2H4). The molar mass of N2H4 is:
Molar mass of N = 14.01 g/mol
Molar mass of H = 1.01 g/mol
Molar mass of N2H4 = (2 * Molar mass of N) + (4 * Molar mass of H) = (2 * 14.01 g/mol) + (4 * 1.01 g/mol) = 32.05 g/mol
Now, we can calculate the number of moles of hydrazine (N2H4):
Number of moles = Mass / Molar mass = 170 g / 32.05 g/mol = 5.308 moles
Since the mole ratio between N2H4 and O2 is 1:1, the number of moles of oxygen (O2) needed is also 5.308 moles.
You don't furnish an equation. Using the following equation
N2H4 + O2 ==> 2H2O + N2
mols N2H4 = grams/molar mass = 170/32 = approx 5 but you need to redo that.
Since it is 1 mol N2H4 to 1 mol O2, mols N2H4 = mols O2.