Multiple Choice
If a match contained 1.00 g of P, how much P4O10 would form if the following equation was obeyed?
___ KClO3 + ___ P → 10 KCl + ___ P4O10
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3. Chemical Reactions
Stoichiometry
Multiple Choice
The combination reaction for the formation of hydrazine is shown below:
4 NH3 (g) + N2 (g) → 3 N2H4 (l)
Determine the number of moles of hydrazine formed when 25.7 g ammonia reacts with excess nitrogen gas.
A
1.13 mol
B
0.567 mol
C
0.881 mol
D
2.81 mol
Verified step by step guidance1
First, calculate the molar mass of ammonia (NH₃). The molar mass is the sum of the atomic masses of nitrogen (N) and hydrogen (H). Use the periodic table to find these values: N = 14.01 g/mol and H = 1.01 g/mol. Therefore, the molar mass of NH₃ is 14.01 + (3 × 1.01) g/mol.
Convert the given mass of ammonia (25.7 g) to moles using the molar mass calculated in the previous step. Use the formula: moles = mass / molar mass.
Use the stoichiometry of the balanced chemical equation to determine the moles of hydrazine (N₂H₄) produced. According to the equation, 4 moles of NH₃ produce 3 moles of N₂H₄. Set up a ratio to find the moles of N₂H₄: (moles of NH₃) × (3 moles N₂H₄ / 4 moles NH₃).
Calculate the moles of hydrazine formed using the ratio from the previous step. This will give you the theoretical yield of N₂H₄ in moles.
Compare your calculated moles of hydrazine with the given options to determine which one matches your result.
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