How many grams of H2 are needed to produce 11.61 grams of NH3?
2N + 3H2-----------> 2NH3
11.44g of NH3*(1 mole/17.03g)=0.6718 moles of NH3
The reaction is 2 moles of NH3: 3 moles of H2
0.6718 moles of NH3*(3 moles of H2/2 moles of NH3)=1.008 moles of H2
1.008 moles of H2*(2.02g/moles)=2.035g of H2
Part B
1.008 moles of H2*(6.022 x 10^23 molecules/mole)=6.068 x 10^23 molecules
To determine the amount of H2 required to produce 11.61 grams of NH3, we need to apply stoichiometry, using the balanced chemical equation for the reaction between H2 and NH3:
N2 + 3H2 → 2NH3
The molar ratio between H2 and NH3 in this equation is 3:2. This means that for every 3 moles of H2, we would expect 2 moles of NH3 to be produced.
First, we need to convert the mass of NH3 to moles:
Molar mass of NH3:
1 mole of N = 14.01 g
3 moles of H = (3 * 1.01 g) = 3.03 g
Total molar mass = 14.01 g + 3.03 g = 17.04 g
Moles of NH3 = mass of NH3 / molar mass of NH3
Moles of NH3 = 11.61 g / 17.04 g/mol ≈ 0.6815 mol
Now, using the molar ratio, we can determine the moles of H2 required:
Moles of H2 = (moles of NH3 * 3) / 2
Moles of H2 = (0.6815 mol * 3) / 2
Moles of H2 ≈ 1.0223 mol
Finally, we can convert the moles of H2 to grams using its molar mass:
Molar mass of H2 = 2.02 g/mol
Mass of H2 = moles of H2 * molar mass of H2
Mass of H2 = 1.0223 mol * 2.02 g/mol ≈ 2.07 g
Therefore, approximately 2.07 grams of H2 are needed to produce 11.61 grams of NH3.
To determine the number of grams of H2 needed to produce 11.61 grams of NH3, you need to use the balanced chemical equation for the reaction.
The balanced chemical equation for the formation of ammonia (NH3) from hydrogen (H2) is:
N2 + 3H2 → 2NH3
From the equation, we can see that 3 moles of H2 are required to produce 2 moles of NH3.
To calculate the number of moles of NH3 produced, we divide the given mass of NH3 (11.61 grams) by its molar mass (17.031 grams/mole):
moles of NH3 = 11.61 grams / 17.031 grams/mole = 0.682 mole
Since the molar ratio of H2 to NH3 is 3:2, we can use this ratio to determine the moles of H2 required:
moles of H2 = (moles of NH3) x (3 moles of H2 / 2 moles of NH3)
= 0.682 mole x (3/2)
= 1.023 mole
Finally, we can convert the moles of H2 to grams by multiplying it by the molar mass of H2 (2.016 grams/mole):
grams of H2 = moles of H2 x molar mass of H2
= 1.023 mole x 2.016 grams/mole
= 2.060 grams
Therefore, approximately 2.060 grams of H2 are needed to produce 11.61 grams of NH3.