Use this equation: N2 + 3 H2 ---> 2 NH3
If 3.00 moles of H2 were used, how many moles of NH3 would be made?
If 0.600 moles of NH3 were produced, how many moles of H2 are required?
just tell me the answer
I'm waiting for that response bro
All of this type question are solved by the factor method using the coefficients as factors. Here is the first one; you see if you can do the second one.
3.00 mols H2 x (2 mols NH3/3 mols H2) = 3.00 x 2/3 = 2.00 mols NH3 produced.
i still don't understand the second
@DrBob222
If 3.00 moles of H2 were used, you would end up with 2.00 moles of NH3. It's like H2 did a magic trick and transformed itself into NH3!
Now, if 0.600 moles of NH3 were produced, you would need 0.900 moles of H2. It's like H2 is the magician's assistant, making NH3 appear out of thin air!
To solve these problems, we need to use the stoichiometry of the chemical reaction.
For the first question:
Given that 3.00 moles of H2 were used, we want to find how many moles of NH3 would be produced.
Looking at the balanced chemical equation: N2 + 3 H2 ---> 2 NH3
We can see that the stoichiometric ratio between H2 and NH3 is 3:2. This means that for every 3 moles of H2, we will produce 2 moles of NH3.
To calculate the moles of NH3 produced, we can use the following conversion:
(3.00 moles H2) x (2 moles NH3 / 3 moles H2) = 2.00 moles NH3
Therefore, if 3.00 moles of H2 were used, 2.00 moles of NH3 would be made.
For the second question:
Given that 0.600 moles of NH3 were produced, we want to find how many moles of H2 are required.
Using the same stoichiometry, we know that the ratio of H2 to NH3 is 3:2. This means that for every 3 moles of H2, we will produce 2 moles of NH3.
To calculate the moles of H2 required, we can use the following conversion:
(0.600 moles NH3) x (3 moles H2 / 2 moles NH3) = 0.900 moles H2
Therefore, if 0.600 moles of NH3 were produced, 0.900 moles of H2 are required.
N2 + 3H2 ==> 2NH3
We have 3.0 mols H2. We can convert that to any thing with the proper factor. The factor is made using the coefficients in the balanced equation.
3.0 mol H2 x factor = mols NH3.
3.0 mols H2 x (2 mol NH3/3 mol H2) = ?
See that mol H2 cancel and leaves mol NH3 which is what you wanted. So what you want to convert TO goes on top and what you are converting FROM goes on the bottom. So 3.0 x 2/3 = 2 mol NH3 produced.
How much N2 was used?
3.0 mols H2 x (1 mol N2/3 mols H2) = 3.0 x 1/3 = 1.0 mol N2 used.
To convert anything to anything it's the
known value x (factor) = new value or
know value x (to/from) = ?