Multiple Choice
Given the balanced equation N2(g) + 3 H2(g) → 2 NH3(g), what is the rate of reaction with respect to [NH3] if the rate of disappearance of H2 is 0.6 mol/L·s?
3. Chemical Reactions
Stoichiometry
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How many grams of Li3N can be formed from 1.75 moles of Li based on the following balanced chemical equation of the reaction? Assume an excess of nitrogen. 6 Li(s) + N2(g) → 2 Li3N(s)
A
20.3 grams
B
58.3 grams
C
29.2 grams
D
116.6 grams
Verified step by step guidance1
Identify the balanced chemical equation: 6 Li(s) + N2(g) → 2 Li3N(s). This equation tells us that 6 moles of lithium react with 1 mole of nitrogen gas to produce 2 moles of lithium nitride.
Determine the mole ratio between lithium and lithium nitride from the balanced equation. The ratio is 6 moles of Li to 2 moles of Li3N, which simplifies to 3 moles of Li to 1 mole of Li3N.
Calculate the moles of Li3N that can be formed from 1.75 moles of Li using the mole ratio. Use the formula: \( \text{moles of Li3N} = \frac{1.75 \text{ moles Li}}{3} \).
Convert the moles of Li3N to grams. First, calculate the molar mass of Li3N by adding the atomic masses of 3 lithium atoms and 1 nitrogen atom. Use the formula: \( \text{grams of Li3N} = \text{moles of Li3N} \times \text{molar mass of Li3N} \).
Perform the multiplication to find the mass of Li3N that can be formed. This will give you the final answer in grams.
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