Nitrogen and hydrogen gases react to form ammonis gas as follows:
N2(g)+3H2(g)-->2NH3(g)
At a certain temperature and pressure, 1.2L of N2 reacts with 3.6L of H2. If all the N2 and H2 are consumed, what volume of NH3 at the same temperature and pressure will be produced?
I'd really appreciate an explanation as to how to go about doing this problem. It looks like it should be simple, but I can't seem to get a firm grasp on it.
on the left, 4 volumes=2volumes on right.
What is 2.4L?
Could you provide more explanation as to where those numbers came from?
First since there
To solve this problem, you will need to use the concept of stoichiometry in chemistry. Stoichiometry is the calculation of reactants and products in chemical reactions.
Step 1: Prepare the balanced chemical equation
The given chemical equation is already balanced: N2(g) + 3H2(g) → 2NH3(g). This means that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3.
Step 2: Calculate the number of moles of N2 and H2 used
To find the number of moles of N2 and H2 used, you need to convert the given volumes to moles using the ideal gas law equation: PV = nRT. As the temperature and pressure are constant, you can use the simplified form PV = n where P is the pressure, V is the volume, and n is the number of moles.
Given:
Volume of N2 = 1.2 L
Volume of H2 = 3.6 L
To convert the volume to moles, you need to know the molar volume of an ideal gas at the given temperature and pressure. Assuming ideal gas behavior, one mole of any gas occupies 22.4 L at standard temperature and pressure (STP).
Moles of N2 = Volume of N2 / Molar volume
Moles of H2 = Volume of H2 / Molar volume
Step 3: Determine the limiting reactant
The limiting reactant is the reactant that will be completely consumed, limiting the amount of product that can be formed. It is crucial in stoichiometry calculations.
To find the limiting reactant, compare the number of moles of N2 and H2 used. The reactant with the lower number of moles used is the limiting reactant.
Step 4: Calculate the moles of NH3 produced
Using the balanced chemical equation, you know that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. Therefore, the ratio of moles between N2 and NH3 is 1:2.
If N2 is the limiting reactant, then the moles of NH3 produced would be 2 times moles of N2 used.
If H2 is the limiting reactant, then the moles of NH3 produced would be 2 times moles of H2 used.
Step 5: Convert moles of NH3 to volume
Finally, convert the moles of NH3 to volume using the ideal gas law equation: Volume = n × Molar volume.
Given:
Molar volume = 22.4 L (at STP)
Volume of NH3 = Moles of NH3 × Molar volume
By following these steps, you should be able to solve the problem and calculate the volume of NH3 produced.