Ammonium perchlorate (NH4CLO4) is the solid rocket fuel that was used by the US space shuttle and is used In the space launch system of the Artemis rocket. It reacts with itself to produce nitrogen gas (N2), chlorine gas (cl2), oxygen gas (O2), water (H20), and a great deal of energy. What mass of nitrogen gas is produced by the reaction of 1.77g of ammonium perchlorate? Round your answer to 3 significant figures
To find the mass of nitrogen gas (N2) produced by the reaction of 1.77g of ammonium perchlorate (NH4ClO4), we first need to determine the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction can be represented as follows:
NH4ClO4 → N2 + 2H2O + 4HClO3
From the balanced equation, we can see that for every 1 mole of NH4ClO4, 1 mole of N2 is produced.
Next, we need to calculate the number of moles of NH4ClO4 in 1.77g of the compound.
Using the molar mass of NH4ClO4:
Molar mass of NH4ClO4 = (1 * 14.01) + (4 * 1.01) + (1 * 35.45) + (4 * 16.00) = 117.49 g/mol
Number of moles of NH4ClO4 = mass / molar mass = 1.77g / 117.49 g/mol = 0.015 moles
Since the stoichiometry of the balanced equation tells us that 1 mole of NH4ClO4 produces 1 mole of N2, the number of moles of N2 produced by the reaction is also 0.015 moles.
Finally, we can calculate the mass of N2 produced using the molar mass of N2:
Molar mass of N2 = (2 * 14.01) = 28.02 g/mol
Mass of N2 = moles of N2 * molar mass of N2 = 0.015 moles * 28.02 g/mol = 0.420 g
Therefore, the mass of nitrogen gas produced by the reaction of 1.77g of ammonium perchlorate is 0.420 grams.