N2(g) + 3H2(g) -> 2NH3(g) at STP

a) How many litres of ammonia gas is produced using 5 litres of H2?
b) How many moles of N2 are needed?

3L H2 produces 2L NH3 -- so 5/3 * 2 = 10/3 L

10/3 L * 1mole/22.4L = 0.15 mole

a) To determine how many liters of ammonia gas is produced using 5 liters of H2, we first need to understand the stoichiometry of the balanced chemical equation.

The balanced equation is:
N2(g) + 3H2(g) -> 2NH3(g)

From the balanced equation, we can see that 3 moles of H2 react to produce 2 moles of NH3.

Now, let's find the number of moles of H2 in 5 liters of H2.
To do this, we need to know the molar volume of a gas at STP, which is 22.4 liters/mol.

The molar volume can be used as a conversion factor to convert between liters and moles of a gas.
So, 5 liters of H2 is equal to (5/22.4) moles of H2.

From the balanced equation, we know that 3 moles of H2 react to produce 2 moles of NH3.
Therefore, (5/22.4) moles of H2 will react to produce [(5/22.4) * 2/3] moles of NH3.

Finally, to convert moles of NH3 to liters, we can multiply by the molar volume at STP:
[(5/22.4) * 2/3] moles of NH3 * 22.4 liters/mole = volume of NH3 in liters.

b) To determine how many moles of N2 are needed, we use the same stoichiometry information from the balanced equation.

From the balanced equation, we can see that 1 mole of N2 reacts to produce 2 moles of NH3.

Since we know the stoichiometric ratio and want to find the number of moles of N2, we can use the following formula:
moles of N2 = (moles of NH3 * ratio of N2 in the balanced equation) / ratio of NH3 in the balanced equation.

From the balanced equation, the ratio of NH3 to N2 is 2:1, which means 2 moles of NH3 are produced for every 1 mole of N2.

Therefore, the number of moles of N2 needed can be calculated as:
moles of N2 = (moles of NH3 * 1) / 2.

Please provide the number of moles of NH3 in order for us to calculate the moles of N2 needed.