Multiple Choice
According to the reaction 2 LiOH + FeCl2 → 2 LiCl + Fe(OH)2, how many moles of Fe(OH)2 can be formed from 175.0 mL of 0.227 M LiOH solution?
3. Chemical Reactions
Stoichiometry
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How many grams of Li3N can be formed from 1.75 moles of Li, assuming an excess of nitrogen? The balanced equation is: 6 Li(s) + N2(g) → 2 Li3N(s).
A
34.9 grams
B
58.3 grams
C
20.3 grams
D
12.5 grams
Verified step by step guidance1
Start by identifying the balanced chemical equation: 6 Li(s) + N2(g) → 2 Li3N(s). This equation tells us the stoichiometric relationship between lithium (Li) and lithium nitride (Li3N).
Determine the molar ratio between Li and Li3N from the balanced equation. According to the equation, 6 moles of Li produce 2 moles of Li3N. Therefore, the molar ratio is 6:2 or 3:1.
Calculate the moles of Li3N that can be formed from 1.75 moles of Li using the molar ratio. Since 3 moles of Li produce 1 mole of Li3N, divide the moles of Li by 3 to find the moles of Li3N: \( \frac{1.75 \text{ moles Li}}{3} \).
Find the molar mass of Li3N. Lithium (Li) has an atomic mass of approximately 6.94 g/mol, and nitrogen (N) has an atomic mass of approximately 14.01 g/mol. Calculate the molar mass of Li3N: \( 3 \times 6.94 + 14.01 = 34.83 \text{ g/mol} \).
Convert the moles of Li3N to grams using its molar mass. Multiply the moles of Li3N by the molar mass of Li3N: \( \text{moles Li3N} \times 34.83 \text{ g/mol} \). This will give you the mass of Li3N that can be formed.
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