객관식
Given the reaction 2 H_2 + O_2 → 2 H_2O, what mass of O_2 (in grams) is required to produce 55.0 grams of H_2O?
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3. Chemical Reactions
Stoichiometry
객관식
Given an excess of nitrogen gas, how many grams of Li3N can be formed from 1.75 moles of Li? (Molar mass of Li3N = 34.83 g/mol)
A
20.3 g
B
10.2 g
C
34.8 g
D
5.83 g
검증된 단계별 안내1
Write the balanced chemical equation for the reaction between lithium (Li) and nitrogen gas (N\_2) to form lithium nitride (Li\_3N). The balanced equation is: \(6\ \mathrm{Li} + \mathrm{N}_2 \rightarrow 2\ \mathrm{Li}_3\mathrm{N}\).
Determine the mole ratio between lithium and lithium nitride from the balanced equation. From the equation, 6 moles of Li produce 2 moles of Li\_3N, so the mole ratio is \(\frac{2}{6} = \frac{1}{3}\) mole of Li\_3N per mole of Li.
Calculate the moles of Li\_3N formed from 1.75 moles of Li using the mole ratio: \(\text{moles of Li}_3\mathrm{N} = 1.75 \times \frac{1}{3}\).
Use the molar mass of Li\_3N (34.83 g/mol) to convert moles of Li\_3N to grams: \(\text{mass of Li}_3\mathrm{N} = \text{moles of Li}_3\mathrm{N} \times 34.83\ \mathrm{g/mol}\).
Perform the multiplication to find the mass of Li\_3N formed from 1.75 moles of Li.
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