How many grams of N2 are needed to produce if 12.0 grams of NH3?
To find the grams of N2 needed to produce 12.0 grams of NH3, we first need to write the balanced chemical equation for the reaction between N2 and H2 to produce NH3:
N2 + 3H2 -> 2NH3
From the balanced equation, we can see that 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3.
Now, we need to calculate the molar mass of NH3:
N = 14.01 g/mol
H = 1.01 g/mol
Molar mass of NH3 = 14.01 g/mol + 3(1.01 g/mol) = 17.02 g/mol
Next, calculate the moles of NH3 produced from 12.0 grams:
moles NH3 = 12.0 g NH3 / 17.02 g/mol = 0.704 moles NH3
Since the ratio of N2 to NH3 is 1:2 in the balanced equation, we need half as many moles of N2 as moles of NH3:
moles N2 = 0.704 moles NH3 / 2 = 0.352 moles N2
Finally, calculate the grams of N2 needed to produce 0.352 moles of N2:
mass N2 = moles N2 * molar mass of N2
mass N2 = 0.352 moles * 28.02 g/mol = 9.86 grams
Therefore, 9.86 grams of N2 are needed to produce 12.0 grams of NH3.